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Chemistry LibreTexts

2A: Basic Atomic Structure (Worksheet)

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  • Page ID 81591

  • Robert Carter
  • University of Massachusetts Boston

Name: ______________________________

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Work in groups on these problems. You should try to answer the questions without referring to your textbook. If you get stuck, try asking another group for help.

The atomic theory of matter is the great organizing principle of chemistry. Atoms are the fundamental building blocks of all matter. The mass relationships between elements and compounds in chemical reactions ultimately relate back to the characteristics of the atoms of which they are composed. To understand how atoms combine to form compounds, you need to understand their basic composition and structure.

Learning Objective

  • Understand the basis for atomic theory
  • Understand the structure of atoms, isotopes, and ions
  • Understand the relationship between the masses of isotopes and the atomic weight of an element
  • Become familiar with the periodic table

Success Criteria

  • Be able to write the standard nuclide notation for an isotope
  • Be able to determine the numbers of fundamental particles in atoms and ions
  • Be able to calculate atomic mass of a mixture of isotopes and percent isotopic composition
  • Be able to categorize elements by position in the periodic table

Law of Definite Proportions

Dalton's Atomic Theory was based in part on the work of the French scientist Joseph Louis Proust in 1799 who discovered what is now called the Law of Definite Proportions (also called the Law of Constant Composition):

A compound is always composed of the same elements in a fixed ratio by weight.

Example : When 200.59 g of mercury reacts completely with 32.066 g sulfur, 232.66 g of red mercury sulfide is produced. What is the percent composition by weight of red mercury sulfide?

\[ \%Hg = \dfrac{200.59\,g}{232.66 \,g} \times 100\% = 86.216 \%Hg \nonumber \]

\[ \%S = \dfrac{32.066\,g}{232.66 \,g} \times 100\% = 13.782 \%Hg \nonumber \]

For every sample of red mercury sulfide the same percent composition by weight is found (the mineral cinnabarite is this compound). It follows from this that a compound of mercury and sulfur with any other percent composition by weight must be a different substance.

Proust's discovery suggested to Dalton that the elements from which compounds are formed must be composed of indivisible units, which combine in specific ways. From this idea, he proposed an atomic theory, which in modern terminology consists of the following points:

  • All matter is composed of atoms.
  • All atoms of an element have the same mass (atomic weight).
  • All atoms of different elements have different masses (i.e., different atomic weights).
  • Atoms are indestructible and indivisible.
  • Compounds are formed when atoms of two or more elements combine.
  • In a compound the relative numbers and kinds of atoms are constant.

Points 2, 3, and 4 are now known to be incorrect , in light of the following later discovered facts:

  • Many elements are composed of a mixture of isotopes, atoms of the same element with different masses.
  • Some atoms of two different elements may have virtually the same mass; these are called isobars.
  • Atoms can be split (fission) or merged (fusion) in nuclear reactions. Some of the mass of atoms is converted to energy in nuclear reactions.

What is the Law of Definite Proportions in your words?

Why Does the Law of Definite Proportions suggest the postulates of Dalton’s atomic theory?

Law of Multiple Proportions

Dalton knew that some pairs of elements could make more than one kind of compound and that the percentages of each element were different in each case. On the basis of his atomic theory he predicted and experimentally verified the Law of Multiple Proportions: If two elements can form more than one compound, then the ratios of the weights of one element in the compounds to a fixed weight of the other element are small whole numbers.

Explain how Dalton’s atomic theory predicts the Law of Multiple Proportions.

Suppose elements X and Y can form two compounds. One compound has as many X atoms as Y atoms (formula \(XY\)), and the other compound has twice as many \(X\) atoms as \(Y\) atoms (formula \(X_2Y\)). What mass ratios would you compare between these compounds to demonstrate the Law of Multiple Proportions? What whole number ratio would be expected between these ratios?

A chemist prepared three different compounds that contain only iodine and fluorine and determined the mass of each element in each compound, as shown below. Calculate the mass of fluorine per gram of iodine in each compound, and explain how your results support atomic theory.

Modern Atomic Theory

Today we know that atoms may be composed of three fundamental particles:

Unit electrical charge is \( 1.6022 \times 10^{-19}\) coulomb (C). The nucleus at the center of the atom contains one or more positively charged protons. All atoms of a given element have the same number of protons , which defines the element's atomic number, given the symbol \(Z\). In addition, the nucleus may contain one or more neutrons, which have approximately the same mass as protons but have no charge. Together, protons and neutrons are known as nucleons . Any atom with a certain number of nucleons is called a nuclide . The number of nucleons defines the nuclide's mass number , given the symbol \(A\):

\[A = \text{number of protons} + \text{number of neutrons } \nonumber \]

Note that the mass number is an integer count of the number of nucleons, and not a statement of an atom's mass. Isotopes of an element have the same atomic number (Z) but have different mass numbers (A), because they have different numbers of neutrons. Isobars are nuclides of different elements (different \(Z\)) with the same mass number (\(A\)). Isobars have nearly the same mass. The standard notation for a nuclide has the form

\[\ce{^{A}_{Z}X} \nonumber \]

where \(X\) is the element's symbol; \(Z\) is its atomic number, equal to the number of protons; and \(A\) is the mass number, equal to the total number of nucleons (protons and neutrons). An electrically neutral atom has the same number of protons as electrons , negatively charged particles that reside outside the nucleus. Atoms may acquire electrical charge by either gaining or losing one or more electrons, thus becoming monatomic ions. Positive ions are cations; negative ions are anions.

\[Atom \rightarrow [Cation]^{n+} + ne^– \nonumber \]

\[Atom + ne^- \rightarrow [Anion]^{n–} \nonumber \]

What is the basis for defining the atomic number (\(Z\)) of an element?

What is the basis for defining the mass number (\(A\)) of a nuclide?

Are Z and A exact or inexact numbers?

How does an atom become a cation or anion?

Does Z or A change in forming an ion? Why or why not?

In some nuclear reactions an atom’s number of protons can change. Is it the same element after such a change?

On the periodic table attached, each block shows the atomic number of the element at the top, above the element’s symbol. With the aid of the periodic table, give the standard nuclide notation for the following isotopes used in medicine: phosphorous-32, chromium-51, cobalt-60, iodine-131.

With the aid of the periodic table, fill in the blanks in the following table:

Mass-Energy Equivalency

Because the masses of atoms are so small, it is more convenient to give nuclide masses in atomic mass units, abbreviated amu or u (the latter is the official SI abbreviation), rather grams. The atomic mass unit is defined as follows:

One atomic mass unit is defined as 1/12 of the mass of \(\ce{^{12}_{6}C}\) atom.

In atomic mass units the fundamental particles have the following masses

  • proton: 1.007277 u
  • neutron: 1.008665 u
  • electron: 0.0005486 u

We cannot use these data to calculate the mass of a given atom, because the mass of a nuclide is not simply the sum of the masses of its fundamental particles. When atoms are formed from protons, neutrons, and electron, some mass is converted into energy, called the binding energy. The mass equivalent of this energy can be calculated from the difference between the measured mass of the nuclide and the sum of the masses of its subatomic particles, using Einstein's famous formula:

\[E = mc^2 \nonumber \]

where \(m\) is the mass converted into energy, and \(c\) is the speed of light in a vacuum.

Because of the existence of isotopes, the masses of individual atoms in a sample of an element may not all be the same. Indeed, with a few exceptions, most naturally occurring samples of an element are mixtures of two or more isotopes in unequal portions. We generally deal with samples containing large numbers of atoms with the usual mix of isotopes for the element, so it is more useful to use an average atomic mass , weighted according to isotopic abundance. By long standing tradition, this average has been called the atomic weight , even though the quantity is actually mass. In general, tabulated values of atomic weights for elements do not represent the mass of a single nuclide, unless the element occurs naturally as only one isotope.

For all elements except fluorine, the atomic weight listed on the periodic table does not correspond to the mass of any nuclide? What does the atomic mass of most elements represent?

The atomic weight listed for fluorine on the periodic table (18.998403 u) does correspond to the mass of a particular nuclide. What does that imply about the isotopic composition of naturally occurring fluorine?

A boron sample found on earth consists of 19.78% \(\ce{^{10}B}\) with atomic mass 10.0129 u and 80.22% \(\ce{^{11}B}\) with atomic mass 11.00931 u. Calculate the atomic weight of naturally occurring boron.

By definition, the mass of \(\ce{^{12}_{6}C}\) atom is exactly 12 u. What is the sum of the masses of the particles (nucleons and electrons) comprising a neutral \ (\ce{^{12}_{6}C}\) atom? Why is the sum not 12 u?

Information In 1869 Dmitri Mendeleev (Russian) and Julius Lothar Meyer (German) independently discovered that when elements are arranged in order of their atomic weights, characteristic properties of certain elements are repeated in other heavier elements at regular intervals in the sequence. From this emerged the first statement of periodic law: The properties of elements are a periodic function of their atomic weights. This ordering, however, seemed to place some elements out of sequence. A better arrangement, based on atomic number, became possible in 1913, when Henry G. J. Moseley found that the atomic numbers of elements could be determined experimentally from their characteristic x-ray frequencies. Today the periodic law is based on atomic numbers, rather than atomic weights:

The properties of elements are a periodic function of their atomic numbers (Z).

In most modern periodic tables, each block for an element shows its atomic number in the first line, the element’s symbol underneath that, and the atomic weight of a naturally occurring sample of the element below its symbol. The following definitions are used in conjunction with the periodic table:

  • group - a column in the periodic table, listing elements that tend to show similar chemical behavior. In North America, groups have been numbered 1 through 8 (or 0) with appended letter designations A or B (e.g., 1A, 3B). The newer I.U.P.A.C. system uses numbers 1 through 18. Although hydrogen, H, is sometimes shown in group 1 (and even group 17), it really belongs to no group, because its chemistry is unique.
  • period - a row in the periodic table. Periods are numbered 1 through 7. main group elements (or representative elements) - members of the A group elements (old North American system); i.e., groups 1A (1) and 2A (2), and 3A (13) through 8A (18) (newer I.U.P.A.C. system designations in parentheses).
  • transition elements - members of the B group elements (old North American system), corresponding to the groups 3 through 12 in the I.U.P.A.C. system. The first, second, and third transition series span these groups in periods 4, 5, and 6, respectively. [Element number 89 (actinium, Ac) in period 7 begins a fourth transition series that would be continued with elements 104 through 112, but these are all unstable, synthetic elements.]
  • lanthanides - elements 58 through 71 in the first row at the bottom of the periodic table (a continuation of period 6). Lanthanum (La) is actually the first element of the third transition series, not a lanthanide.
  • actinides - elements 90 through 103 in the second row at the bottom of the periodic table (a continuation of period 7). Actinium (Ac) is actually the first element of an incomplete fourth transition series, not an actinide.

There are three categories of elements: metals, nonmetals, and metalloids, defined as follows:

  • metals - elements in groups 1A (1) and 2A (2), the transition elements, the lanthanides and actinides, and the heavier elements in groups 3A (13) through 5A (15) that lie below the stair step shown on some periodic tables. At room temperature metals are shiny solids (except mercury and gallium above 29.78o C, which are liquids) that are malleable, ductile, and conductive of heat and electricity. Metals characteristically are cations in their ionic compounds.
  • nonmetals - the elements in groups 4A (14) through 7A (17) that lie above the stair step on some periodic tables. Individual nonmetals may be either solids, liquids, or gases at room temperature. They are poor conductors of heat and electricity. Nonmetals characteristically are anions, when existing as monatomic ions in ionic compounds. When combined with other nonmetals, they typically form molecular compounds or complex ions.
  • metalloids - the elements B, Si, Ge, As, Sb, Te, Po, At, which lie along the stair step shown on some periodic tables. All are solids with semi-metallic properties. They show poorer conductivity relative to metals and may be semiconductors (e.g., Si and Ge).

What information about an element is provided in the box for that element in the periodic table?

What determines the sequence of elements from the first to the last?

What is the difference between a group and a period?

Where are the metals, nonmetals, and metalloids located?

Qre the majority of elements metals, nonmetals, or metalloids?

Does hydrogen belong to group 1? Why or why not? Exercises

Write the name, symbol, atomic number and average mass for each of the following, and indicate whether the element is metal, nonmetal, or metalloid:

  • The group 2 element in period 3
  • The group 16 element in period 2
  • The group 15 element in period 4

Write the name and symbol of the element that has 48 electrons.

Name the elements with properties similar to chlorine, Cl.

Give the symbols and names of elements 57 and 72 in the period 6. Why are they adjacent to each other in the periodic table? Problem

Chlorine consists of \(\ce{^{35}Cl}\) with a mass of 34.96885 u and \(\ce{^{37}Cl}\) with a mass of 36.96590 u. The atomic weight of chlorine is 35.453 u. What is the percent abundance of each isotope?

Chemistry Worksheets Class 11 on Chapter 3 Classification of Elements and Periodicity in Properties with Answers - Set 1

Element are the fundamental building blocks that make up all of the material matter in our environment. Initially, 31 chemical elements were identified in 1800. In 1865, a few technological advances led to the discovery of around 63 more elements. As a result, the periodic classification of elements became necessary. Currently, 118 elements are known to us, and some of these chemical elements are artificial.

Download Class 11 Chemistry Worksheet on Chapter 3 Classification of Elements and Periodicity in Properties Set 1 PDF .

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Chemistry Worksheets Class 11 on Chapter 3 Classification of Elements and Periodicity in Properties Set 1

CBSE Class 11 Chemistry Chapter 3 Classification of Elements and Periodicity in Properties – Set 1

Q-1: What happens when a neutral atom is converted into an anion?

a) Atomic weight increases

b) Atomic weight decreases

c) Size increases

d) Size decreases

Q-2: The element with the highest affinity for electrons will belong to

a) Period 2, Group 17

b) Period 2, Group 18

c) Period 3, Group 17

d) Period 2, Group 1

Q-3: Which of the following is not a representative element?

Q-4: Find the incorrect statement.

a) For group 2, the valence electron and valency are identical.

b) Metal, non-metal, and metalloids are all present in P-block elements.

c) Helium (He) is the only noble gas with two valence electrons.

d) The smallest element on the periodic table is He.

Q-5: The symbol of an element with atomic number Z = 109 is

Q-6: Which among the following will have the largest atomic radii based on their positions in the periodic table?

Be, N, O, Ne

Q-7: Is the electronegativity of an atom constant?

Q-8: Which element among the following has the highest positive electron gain enthalpy? Neon, Nitrogen, and Fluorine

Q-9: Give the inert gas atom’s name and atomic number in which the total number of d-electrons equals the difference in numbers of total p and s-electrons.

Q-10: Show by chemical reaction with water that K 2 O is a basic oxide and Cl 2 O 7 is an acidic oxide.

Q-11: What would be the atomic number for the following if they were discovered in the future?

(i) Next alkali metal

(ii) Next alkaline earth metal

(iii) Next inert gas

Q-12: Give the general valence shell electronic configuration of transition elements and some characteristics. Also, tell the block to which they belong and why?

Q-13: Do the non-metallic character exhibited by the halogens have any relation to ionisation enthalpy?

Q-14: Why do s-block elements act as strong reducing agents?

Q-15: What will be the fluorine atom’s atomic radius in a covalently bound fluorine molecule with a 128 pm internuclear distance?

Q-16: Why are there only 14 lanthanides and only 14 actinides?

a) What do you understand by shielding effect or screening effect? How does it affect the ionisation enthalpy?

b) Why can Na not exhibit a +2 oxidation state?

Q-18: Li < Na < K < Rb < Cs are in increasing order of reactivity in group 1, while F > Cl > Br > I are in that group 17. Explain.

Q-19: What is the diagonal relationship? What are the main reasons for the anomalous behaviour of the elements belonging to the second period?

Q-20: The amount of energy released when 1 × 10 10 atoms of bromine in vapour state are converted to Br – ions according to the equation, Br(g) + e – → Br – (g) is 60.90 × 10 -10 J. Calculate the electron gain enthalpy of bromine atom in terms of eV per atom.

Download the PDF to access answers to the Chemistry Worksheet for Class 11 Chemistry Chapter 3 Classification of Elements and Periodicity in Properties Set – 1.

  • Classification of Elements and Periodicity in Properties
  • Periodic Classification of Elements
  • Periodic Properties of Elements and Their Significance
  • Periodic Table
  • Modern Periodic Law
  • Important Questions for Class 11 Chemistry Chapter 3 Classification of Elements and Periodicity in Properties
  • Class 11 Chemistry Chapter 3 Classification of Elements and Periodicity in Properties
  • Chemistry Concept Questions and Answers

periodicity chemistry worksheet answer key

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  • Introduction
  • 1.1 Chemistry in Context
  • 1.2 Phases and Classification of Matter
  • 1.3 Physical and Chemical Properties
  • 1.4 Measurements
  • 1.5 Measurement Uncertainty, Accuracy, and Precision
  • 1.6 Mathematical Treatment of Measurement Results
  • Key Equations
  • 2.1 Early Ideas in Atomic Theory
  • 2.2 Evolution of Atomic Theory
  • 2.3 Atomic Structure and Symbolism
  • 2.4 Chemical Formulas
  • 3.1 Electromagnetic Energy
  • 3.2 The Bohr Model
  • 3.3 Development of Quantum Theory
  • 3.4 Electronic Structure of Atoms (Electron Configurations)
  • 3.5 Periodic Variations in Element Properties
  • 3.6 The Periodic Table
  • 3.7 Ionic and Molecular Compounds
  • 4.1 Ionic Bonding
  • 4.2 Covalent Bonding
  • 4.3 Chemical Nomenclature
  • 4.4 Lewis Symbols and Structures
  • 4.5 Formal Charges and Resonance
  • 4.6 Molecular Structure and Polarity
  • 5.1 Valence Bond Theory
  • 5.2 Hybrid Atomic Orbitals
  • 5.3 Multiple Bonds
  • 5.4 Molecular Orbital Theory
  • 6.1 Formula Mass
  • 6.2 Determining Empirical and Molecular Formulas
  • 6.3 Molarity
  • 6.4 Other Units for Solution Concentrations
  • 7.1 Writing and Balancing Chemical Equations
  • 7.2 Classifying Chemical Reactions
  • 7.3 Reaction Stoichiometry
  • 7.4 Reaction Yields
  • 7.5 Quantitative Chemical Analysis
  • 8.1 Gas Pressure
  • 8.2 Relating Pressure, Volume, Amount, and Temperature: The Ideal Gas Law
  • 8.3 Stoichiometry of Gaseous Substances, Mixtures, and Reactions
  • 8.4 Effusion and Diffusion of Gases
  • 8.5 The Kinetic-Molecular Theory
  • 8.6 Non-Ideal Gas Behavior
  • 9.1 Energy Basics
  • 9.2 Calorimetry
  • 9.3 Enthalpy
  • 9.4 Strengths of Ionic and Covalent Bonds
  • 10.1 Intermolecular Forces
  • 10.2 Properties of Liquids
  • 10.3 Phase Transitions
  • 10.4 Phase Diagrams
  • 10.5 The Solid State of Matter
  • 10.6 Lattice Structures in Crystalline Solids
  • 11.1 The Dissolution Process
  • 11.2 Electrolytes
  • 11.3 Solubility
  • 11.4 Colligative Properties
  • 11.5 Colloids
  • 12.1 Spontaneity
  • 12.2 Entropy
  • 12.3 The Second and Third Laws of Thermodynamics
  • 12.4 Free Energy
  • 13.1 Chemical Equilibria
  • 13.2 Equilibrium Constants
  • 13.3 Shifting Equilibria: Le Châtelier’s Principle
  • 13.4 Equilibrium Calculations
  • 14.1 Brønsted-Lowry Acids and Bases
  • 14.2 pH and pOH
  • 14.3 Relative Strengths of Acids and Bases
  • 14.4 Hydrolysis of Salts
  • 14.5 Polyprotic Acids
  • 14.6 Buffers
  • 14.7 Acid-Base Titrations
  • 15.1 Precipitation and Dissolution
  • 15.2 Lewis Acids and Bases
  • 15.3 Coupled Equilibria
  • 16.1 Review of Redox Chemistry
  • 16.2 Galvanic Cells
  • 16.3 Electrode and Cell Potentials
  • 16.4 Potential, Free Energy, and Equilibrium
  • 16.5 Batteries and Fuel Cells
  • 16.6 Corrosion
  • 16.7 Electrolysis
  • 17.1 Chemical Reaction Rates
  • 17.2 Factors Affecting Reaction Rates
  • 17.3 Rate Laws
  • 17.4 Integrated Rate Laws
  • 17.5 Collision Theory
  • 17.6 Reaction Mechanisms
  • 17.7 Catalysis
  • 18.1 Periodicity
  • 18.2 Occurrence and Preparation of the Representative Metals
  • 18.3 Structure and General Properties of the Metalloids
  • 18.4 Structure and General Properties of the Nonmetals
  • 18.5 Occurrence, Preparation, and Compounds of Hydrogen
  • 18.6 Occurrence, Preparation, and Properties of Carbonates
  • 18.7 Occurrence, Preparation, and Properties of Nitrogen
  • 18.8 Occurrence, Preparation, and Properties of Phosphorus
  • 18.9 Occurrence, Preparation, and Compounds of Oxygen
  • 18.10 Occurrence, Preparation, and Properties of Sulfur
  • 18.11 Occurrence, Preparation, and Properties of Halogens
  • 18.12 Occurrence, Preparation, and Properties of the Noble Gases
  • 19.1 Occurrence, Preparation, and Properties of Transition Metals and Their Compounds
  • 19.2 Coordination Chemistry of Transition Metals
  • 19.3 Spectroscopic and Magnetic Properties of Coordination Compounds
  • 20.1 Nuclear Structure and Stability
  • 20.2 Nuclear Equations
  • 20.3 Radioactive Decay
  • 20.4 Transmutation and Nuclear Energy
  • 20.5 Uses of Radioisotopes
  • 20.6 Biological Effects of Radiation
  • 21.1 Hydrocarbons
  • 21.2 Alcohols and Ethers
  • 21.3 Aldehydes, Ketones, Carboxylic Acids, and Esters
  • 21.4 Amines and Amides
  • A | The Periodic Table
  • B | Essential Mathematics
  • C | Units and Conversion Factors
  • D | Fundamental Physical Constants
  • E | Water Properties
  • F | Composition of Commercial Acids and Bases
  • G | Standard Thermodynamic Properties for Selected Substances
  • H | Ionization Constants of Weak Acids
  • I | Ionization Constants of Weak Bases
  • J | Solubility Products
  • K | Formation Constants for Complex Ions
  • L | Standard Electrode (Half-Cell) Potentials
  • M | Half-Lives for Several Radioactive Isotopes

The spectrum consists of colored lines, at least one of which (probably the brightest) is red.

3.233 × × 10 −19 J; 2.018 eV

ν = 4.568 × × 10 14 s −1 ; λ = 656.3 nm; Energy mol −1 = 1.823 × × 10 5 J mol −1 ; red

(a) λ = 8.69 × × 10 −7 m; E = 2.29 × × 10 −19 J; (b) λ = 4.59 × × 10 −7 m; E = 4.33 × × 10 −19 J; The color of (a) is red; (b) is blue.

E = 9.502 × × 10 −15 J; ν = 1.434 × × 10 19 s −1

Red: 660 nm; 4.54 × × 10 14 Hz; 3.01 × × 10 −19 J. Green: 520 nm; 5.77 × × 10 14 Hz; 3.82 × × 10 −19 J. Blue: 440 nm; 6.81 × × 10 14 Hz; 4.51 × × 10 −19 J. Somewhat different numbers are also possible.

5.49 × × 10 14 s −1 ; no

Quantized energy means that the electrons can possess only certain discrete energy values; values between those quantized values are not permitted.

2.856 eV 2.856 eV

−8.716 × × 10 −18 J

−3.405 × × 10 −20 J

1.471 × × 10 −17 J

Both involve a relatively heavy nucleus with electrons moving around it, although strictly speaking, the Bohr model works only for one-electron atoms or ions. According to classical mechanics, the Rutherford model predicts a miniature “solar system” with electrons moving about the nucleus in circular or elliptical orbits that are confined to planes. If the requirements of classical electromagnetic theory that electrons in such orbits would emit electromagnetic radiation are ignored, such atoms would be stable, having constant energy and angular momentum, but would not emit any visible light (contrary to observation). If classical electromagnetic theory is applied, then the Rutherford atom would emit electromagnetic radiation of continually increasing frequency (contrary to the observed discrete spectra), thereby losing energy until the atom collapsed in an absurdly short time (contrary to the observed long-term stability of atoms). The Bohr model retains the classical mechanics view of circular orbits confined to planes having constant energy and angular momentum, but restricts these to quantized values dependent on a single quantum number, n . The orbiting electron in Bohr’s model is assumed not to emit any electromagnetic radiation while moving about the nucleus in its stationary orbits, but the atom can emit or absorb electromagnetic radiation when the electron changes from one orbit to another. Because of the quantized orbits, such “quantum jumps” will produce discrete spectra, in agreement with observations.

Both models have a central positively charged nucleus with electrons moving about the nucleus in accordance with the Coulomb electrostatic potential. The Bohr model assumes that the electrons move in circular orbits that have quantized energies, angular momentum, and radii that are specified by a single quantum number, n = 1, 2, 3, …, but this quantization is an ad hoc assumption made by Bohr to incorporate quantization into an essentially classical mechanics description of the atom. Bohr also assumed that electrons orbiting the nucleus normally do not emit or absorb electromagnetic radiation, but do so when the electron switches to a different orbit. In the quantum mechanical model, the electrons do not move in precise orbits (such orbits violate the Heisenberg uncertainty principle) and, instead, a probabilistic interpretation of the electron’s position at any given instant is used, with a mathematical function ψ called a wavefunction that can be used to determine the electron’s spatial probability distribution. These wavefunctions, or orbitals, are three-dimensional stationary waves that can be specified by three quantum numbers that arise naturally from their underlying mathematics (no ad hoc assumptions required): the principal quantum number, n (the same one used by Bohr), which specifies shells such that orbitals having the same n all have the same energy and approximately the same spatial extent; the angular momentum quantum number l , which is a measure of the orbital’s angular momentum and corresponds to the orbitals’ general shapes, as well as specifying subshells such that orbitals having the same l (and n ) all have the same energy; and the orientation quantum number m , which is a measure of the z component of the angular momentum and corresponds to the orientations of the orbitals. The Bohr model gives the same expression for the energy as the quantum mechanical expression and, hence, both properly account for hydrogen’s discrete spectrum (an example of getting the right answers for the wrong reasons, something that many chemistry students can sympathize with), but gives the wrong expression for the angular momentum (Bohr orbits necessarily all have non-zero angular momentum, but some quantum orbitals [ s orbitals] can have zero angular momentum).

n determines the general range for the value of energy and the probable distances that the electron can be from the nucleus. l determines the shape of the orbital. m 1 determines the orientation of the orbitals of the same l value with respect to one another. m s determines the spin of an electron.

(a) 2 p ; (b) 4 d ; (c) 6 s

(a) 3 d; (b) 1 s; (c) 4 f

(a) x. 2, y. 2, z. 2; (b) x. 1, y. 3, z. 0; (c) x. 4 0 0 1 2 , 1 2 , y. 2 1 0 1 2 , 1 2 , z. 3 2 0 1 2 ; 1 2 ; (d) x. 1, y. 2, z. 3; (e) x. l = 0, m l = 0, y. l = 1, m l = –1, 0, or + 1, z. l = 2, m l = –2, –1, 0, +1, +2

For example, Na + : 1 s 2 2 s 2 2 p 6 ; Ca 2+ : 1 s 2 2 s 2 2 p 6 3 s 2 3 p 6 ; Sn 2+ : 1 s 2 2 s 2 2 p 6 3 s 2 3 p 6 3 d 10 4 s 2 4 p 6 4 d 10 5 s 2 ; F – : 1 s 2 2 s 2 2 p 6 ; O 2– : 1 s 2 2 s 2 2 p 6 ; Cl – : 1 s 2 2 s 2 2 p 6 3 s 2 3 p 6 .

(a) 1 s 2 2 s 2 2 p 3 ; (b) 1 s 2 2 s 2 2 p 6 3 s 2 3 p 2 ; (c) 1 s 2 2 s 2 2 p 6 3 s 2 3 p 6 4 s 2 3 d 6 ; (d) 1 s 2 2 s 2 2 p 6 3 s 2 3 p 6 4 s 2 3 d 10 4 p 6 5 s 2 4 d 10 5 p 4 ; (e) 1 s 2 2 s 2 2 p 6 3 s 2 3 p 6 4 s 2 3 d 10 4 p 6 5 s 2 4 d 10 5 p 6 6 s 2 4 f 9

The charge on the ion.

Rb + , Se 2−

Although both (b) and (c) are correct, (e) encompasses both and is the best answer.

1 s 2 2 s 2 2 p 6 3 s 2 3 p 6 4 s 2 3 d 10 4 p 6 5 s 2 4 d 10 5 p 6 6 s 2 4 f 14 5 d 10

Co has 27 protons, 27 electrons, and 33 neutrons: 1 s 2 2 s 2 2 p 6 3 s 2 3 p 6 4 s 2 3 d 7 . I has 53 protons, 53 electrons, and 78 neutrons: 1 s 2 2 s 2 2 p 6 3 s 2 3 p 6 3 d 10 4 s 2 4 p 6 4 d 10 5 s 2 5 p 5 .

Rb < Li < N < F

Mg < Ca < Rb < Cs

Si 4+ < Al 3+ < Ca 2+ < K +

Mg 2+ < K + < Br – < As 3–

(a) metal, inner transition metal; (b) nonmetal, representative element; (c) metal, representative element; (d) nonmetal, representative element; (e) metal, transition metal; (f) metal, inner transition metal; (g) metal, transition metal; (h) nonmetal, representative element; (i) nonmetal, representative element; (j) metal, representative element

(a) He; (b) Be; (c) Li; (d) O

(a) krypton, Kr; (b) calcium, Ca; (c) fluorine, F; (d) tellurium, Te

(a) 11 23 Na 11 23 Na ; (b) 54 129 Xe 54 129 Xe ; (c) 33 73 As 33 73 As ; (d) 88 226 Ra 88 226 Ra

Ionic: KCl, MgCl 2 ; Covalent: NCl 3 , ICl, PCl 5 , CCl 4

(a) covalent; (b) ionic, Ba 2+ , O 2− ; (c) ionic, NH 4 + , NH 4 + , CO 3 2− ; CO 3 2− ; (d) ionic, Sr 2+ , H 2 PO 4 − ; H 2 PO 4 − ; (e) covalent; (f) ionic, Na + , O 2−

(a) CaS; (b) (NH 4 ) 2 SO 4 ; (c) AlBr 3 ; (d) Na 2 HPO 4 ; (e) Mg 3 (PO 4 ) 2

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Printable Chemistry Worksheets

Free pdf Worksheets to Download or Print

  • Chemical Laws
  • Periodic Table
  • Projects & Experiments
  • Scientific Method
  • Biochemistry
  • Physical Chemistry
  • Medical Chemistry
  • Chemistry In Everyday Life
  • Famous Chemists
  • Activities for Kids
  • Abbreviations & Acronyms
  • Weather & Climate
  • Ph.D., Biomedical Sciences, University of Tennessee at Knoxville
  • B.A., Physics and Mathematics, Hastings College

This is a collection of chemistry worksheets in pdf format. The answers to the questions are available on separate worksheets so you can fill them out and then check your work. Please feel free to download these to your computer, print them, and use them as hand-outs.

  • Metals, Nonmetals, and Metalloids Worksheet
  • Metric to English Conversions Worksheet
  • Metric to English Conversions Answers
  • Metric to Metric Conversions Worksheet
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  • Temperature Conversions Worksheet
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  • Temperature Conversions Worksheet #2
  • Temperature Conversions Answers #2
  • Moles to Grams Conversions Worksheet
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  • Formula or Molar Mass Worksheet
  • Formula or Molar Mass Worksheet Answers
  • Practicing Balancing Chemical Equations - Worksheet
  • Balancing Chemical Equations - Answers
  • Practicing Balancing Chemical Equations - Worksheet #2
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  • Balancing Equations - Worksheet #4
  • Balancing Equations - Answer Key #4
  • Common Acid Names & Formulas - Worksheet
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  • Practice Calculations with Moles - Worksheet
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  • Gas Laws Answers - Shown Work
  • Limiting Reagent - Worksheet
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  • Calculating Molarity - Worksheet
  • Calculating Molarity - Answers
  • Balancing Redox Reactions - Worksheet
  • Balancing Redox Reactions - Answers
  • Printable Element Crossword
  • Printable Element Crossword - Answers
  • Chemical Names to Chemical Formulas - Worksheet
  • Chemical Names to Chemical Formulas - Answer Key
  • Chemical Formulas to Chemical Names - Worksheet
  • Chemical Formulas to Chemical Names - Answer Key
  • Chemistry Element Word Search

Printable Periodic Tables

Here are some printable periodic tables to help you out, also in pdf format.

  • Color Printable Periodic Table - Pretty much everything you need that can fit on a page and still be readable. Color table with atomic numbers, element symbols, element names, atomic weights, periods, and groups. [ 2013 Edition ] [ 2012 Edition ]
  • Black/white Printable Periodic Table - Black/white table with atomic numbers, element symbols, element names, atomic weights, periods. [ 2013 Edition ] [ 2012 Edition ]
  • Blank Printable Periodic Table - Fill in the boxes yourself.
  • Electron Configuration Periodic Table - Periodic table that lists the electron configurations for each element.
  • Color Printable Periodic Table - Color table with atomic numbers, element symbols, atomic weights, periods, and groups. (no names)
  • Basic Printable Periodic Table - Black/white table with atomic numbers, element symbols, atomic weights, periods. (no names)
  • Basic Periodic Table with Element Names - Black/white table with element symbols, names, atomic numbers, and periods. (no weights)
  • Basic Periodic Table with Element Names (color) - Color periodic table with element symbols, names, atomic numbers, periods, and groups. (no weights)

The atomic weights given on these tables are the most recent (2007) values as accepted by the IUPAC.

Printable Scientific Method Flow Chart

This is a flow chart of the steps of the scientific method, available as a PDF file:

  • Scientific Method PDF

Also available is a PDF of a pie chart of the elemental composition of the human body .

  • A List of Common General Chemistry Problems
  • Printable Periodic Tables (PDF)
  • How to Balance Equations - Printable Worksheets
  • 20 Practice Chemistry Tests
  • Overview of High School Chemistry Topics
  • Molar Mass Example Problem
  • Periodic Table for Kids
  • Clickable Periodic Table of the Elements
  • Topics Typically Covered in Grade 11 Chemistry
  • Balancing Chemical Equations
  • Chemistry Elements Word Search Puzzles With Answers
  • Empirical Formula: Definition and Examples
  • Teach Yourself Chemistry Today
  • A List of the Elements of the Periodic Table
  • How to Use a Periodic Table of Elements
  • Why Is the Periodic Table Important?

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Periodic Table Questions and Answers

Periodic Table Questions and Answers

The periodic table is an important tool in chemistry, so there are many periodic table questions that people have. Here are some common questions, with answers in simple, down-to-Earth language that you can understand, even if you’re not a scientist.

What Is the Periodic Table?

Of course, the most basic question is “What is the periodic table?” The simple answer is that it is a chart that shows all of the chemical elements and basic facts about them, that orders the elements by increasing atomic number and common properties. The atomic number is the number of protons in every atom of the element. The number of neutrons in the atom changes its isotope, but not its element. Similarly, the number of electrons changes the ion , but not the element.

What Are Groups and Periods in the Periodic Table?

The way the periodic table organizes elements by properties is by putting them in rows, which are called periods, and columns, which are called groups . Elements in a period have the same outer electron shell, which gives them some common characteristics. Elements in a group have number of outer or valence electrons , again, giving them common properties.

What Are Periodic Table Trends or Periodicity?

Organizing the table with groups and periods makes certain trends in element properties apparent. In other words, the table displays periodicity (hence its name).

There are several periodic table trends in properties, but the key ones are atomic radius, electronegativity, electron affinity, and ionization energy:

  • Atomic radius is the size of an electrically neutral atom of an element. In increases moving down a group (column) because the atom gains a new electron shell. It decreases moving from left to right across a period (row) because adding protons (increasing atomic number) attracts and draws the electrons in more tightly.
  • Electronegativity is a measure of how easily an atom attracts electrons that can form a chemical bond. It increases moving left to right (except for the noble gases) and mostly decreases moving down a group.
  • Electron affinity is related to electronegativity. It is the energy change that occurs when a neutral atom accepts an electron. It increases moving across a period, but does not always decrease moving down a group.
  • Ionization energy is the energy required to remove an electron from an atom. It increases moving across a period and decreases moving down a group.

There are other also other trends, such as ionic radius, covalent radius, and metallicity.

Who Invented the Periodic Table?

While lots of scientists have made periodic tables over the years, the one that most closely resembles the table we use today was formulated by Dmitri Mendeleev. So, Mendeleev is considered the “ inventor of the periodic table .” His 1869 table differed from the modern table in that it ordered elements by increasing atomic weight instead of atomic number. But, he made the table before protons were discovered. For the most part, using atomic weight instead of atomic number produces the same table.

Why Are the Noble Gases So Inert?

While the noble gases sometimes do participate in chemical reactions, they are mostly unreactive and are exceptions to periodic table trends. The reason is that atoms of elements of this group have stable valence electron shells . In other words, the noble gas atoms become less stable if they lose or gain electrons.

Why Are the Halogens So Reactive?

The halogens (fluorine, chlorine, iodine, etc.) are as reactive as the noble gases are stable. This group is right next to the noble gases, so why is it so reactive? The reason is that they are only one electron away from having a stable configuration. Forming chemical bonds gives the halogens this stability.

What Are the Periodic Table Groups?

While the periods of the periodic table just have numbers corresponding to their rows, the periodic table groups have both numbers and names. Probably the names arose because of the different numbering systems for the groups. The groups are the alkali metals, alkaline earth metals, transition metals, basic metals, metalloids, nonmetals, halogens, and noble gases. The lanthanide and actinide groups are actually a subset of the transition metals.

More Periodic Table Questions

Do you have unanswered periodic table questions? Leave a comment! If it’s a common question, I’ll add it to this article.

  • Bury, Charles R. (July 1921). “Langmuir’s Theory of the Arrangement of Electrons in Atoms and Molecules”. Journal of the American Chemical Society . 43(7): 1602–1609. doi: 10.1021/ja01440a023
  • Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. ISBN 978-0-08-037941-8.
  • Petrucci, Ralph H.; Harwood, William S.; Herring, F. Geoffrey (2002). General Chemistry: Principles and Modern Applications (8th ed.). Upper Saddle River, N.J: Prentice Hall. ISBN 978-0-13-014329-7.
  • Scerri, Eric. 2020. The Periodic Table, Its Story and Its Significance (2nd edition). New York: Oxford University Press. ISBN 978-0190914363.

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  1. PDF SCPS Chemistry Worksheet

    1. Which are metals? Circle your answers: C, Na, F, Cs, Ba, Ni Which metal in the list above has the most metallic character? Explain. Cesium - as the largest atom, the lowest ionization energy and the most reactivity with nonmetals. This can be determined by its position lowest in the alkali metal group. 2.

  2. PDF Chemistry: The Periodic Table and Periodicity

    1. By what property did Mendeleev arrange the elements? 2. By what property did Moseley suggest that the periodic table be arranged? 3. What is the periodic law? 4. What is a period? How many are there in the periodic table? 5. What is a group (also called a family)? How many are there in the periodic table? 6.

  3. 10A: Periodic Trends (Worksheet)

    The following plot shows how atomic radii vary through the periodic table. Across the periodic table, sizes of atoms show the following trends, with many irregularities: Size increases down a group. The outermost electrons are in successively more extensive orbitals as n increases. Size decreases across a period.

  4. 2A: Basic Atomic Structure (Worksheet)

    [Element number 89 (actinium, Ac) in period 7 begins a fourth transition series that would be continued with elements 104 through 112, but these are all unstable, synthetic elements.] lanthanides - elements 58 through 71 in the first row at the bottom of the periodic table (a continuation of period 6). Lanthanum (La) is actually the first ...

  5. PDF Answer Keys for Unit 2

    The period (row) number of the clement is the same as the number of elect shells. As you go down the periodic table, from one period to the next, the number of electron shells increases by one. In the first period, the atoms have electrons in only one shell. In the fourth period, the atoms have electrons in four shells.

  6. PDF Atomic Structure & Periodicity FR worksheet KEY

    Microsoft Word - Atomic Structure & Periodicity FR worksheet KEY 1980 2 points 1s2 2s22p6 3s23p6 4s23d104p3 2 points for the two electrons in the 4s: 4, 0, 0, +1/2 and 4, 0, 0, - 1/2 for the three electrons in the 4p: 4, 1, -1, +1/2; 4, 1, 0, +1/2 and 4, 1, +1, +1/2 2 points Paramagnetic. It has three unpaired electrons. 2 points

  7. PDF SCPS Chemistry Worksheet ΠPeriodicity

    a. period b. group c. both d. neither. 2. In any ___, the number of electrons between the nucleus and the outer energy level is the same. a. period b. group c. both d. neither. 3. Within a ____, the nucleus has a stronger ability to pull on the outermost (valence) electrons in elements of high atomic number.

  8. Class 11 Chemistry Worksheet on Chapter 3 Classification of Elements

    Q-1: What happens when a neutral atom is converted into an anion? a) Atomic weight increases b) Atomic weight decreases c) Size increases d) Size decreases Q-2: The element with the highest affinity for electrons will belong to a) Period 2, Group 17 b) Period 2, Group 18 c) Period 3, Group 17 d) Period 2, Group 1

  9. Answer Key Chapter 3

    1. The spectrum consists of colored lines, at least one of which (probably the brightest) is red. 3. 3.15 m 5. 3.233 × 10 −19 J; 2.018 eV 7. ν = 4.568 × 10 14 s −1; λ = 656.3 nm; Energy mol −1 = 1.823 × 10 5 J mol −1; red 9.

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    View Homework Help - Periodicity Chemistry Worksheet-1.docx from FLVS 101 at West Orange High, West Orange. Periodicity Chemistry Worksheet A. Periodic table 1. Which are metals? ... Nuclear Chemistry - Worksheet ANSWER KEY.pdf. Solutions Available. University of Waterloo. CHEM 240. homework. pre lab 3.pdf. Solutions Available. San Jose State ...

  11. Free PDF Chemistry Worksheets To Download or Print

    This is a downloadable soft colored periodic table of the elements which shows atomic number, element symbol, element name and atomic mass. Todd Helmenstine By Anne Marie Helmenstine, Ph.D. Updated on May 30, 2019 This is a collection of chemistry worksheets in pdf format.

  12. Periodic Table Worksheet

    Students use a periodic table to complete the missing information on 20 element cells. The PDF of this worksheet includes a copy of a printable black and white periodic table. The included periodic table can be downloaded separately here.. The answer key can be found on the next page.. For more practice, check out Periodic Table Worksheet #2.It has the same format, just different element cells.

  13. PDF 5 The Periodic Law

    SHORT ANSWER Use this periodic table to answer the following questions in the space provided. 1. Identify the element and write the noble-gas notation for each of the following: a. the Group 14 element in Period 4 Ge; [Ar]3d104s 24p b. the only metal in Group 15 Bi; [Xe]4f145d106s26p3 c. the transition metal with the smallest atomic mass Sc ...

  14. Chemistry Worksheets and Handouts (PDF for Printing)

    Reading periodic table element information Worksheet #1 [ PDF ] [ Answers] Worksheet #2 [ PDF ] [ Answers] Scientific Notation [ PDF ] [ Answers] Significant digits Rules [ PDF ] [ Answers] Addition and subtraction [ PDF ] [ Answers]

  15. D4 D5 Periodicity Chemistry KEY

    Explain. Ca+2 - Calcium has 2 valence electrons, it will lose 2 electrons Name two more elements with that oxidation number and explain your choice. Any of the two: Be, Mg, Se, Ba, Ra - Same valence electrons / same family What element in period 3 is a metalloid? When element with atomic number 118 is discovered, what family will it be in?

  16. PeriodicityWksht Key

    Na b) Which has the highest electron affinity? O c) Place the elements in order of increasing ionization energy. Na Mg P O lowest highest 9) Explain each answer briefly. a) Place the following elements in order of increasing ionization energy: F, O, and S. S<O<F : Ionization energy increases moving upwards in a group and right in a period.

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    Answerkey for Periodic Table Practice Worksheet Prof Simonyan name date reading the periodic table key list the atomic numbers of the elements in period 10 list ... Sig fg wrksht KEY - Answer key for practice significant figures worksheet Prof Simonyan. ... Element Symbol Atomic Number Period Group sodium Na 11 3 1 oxygen O 8 2 16 krypton Kr 36 ...

  18. Periodic Table Questions and Answers

    Of course, the most basic question is "What is the periodic table?". The simple answer is that it is a chart that shows all of the chemical elements and basic facts about them, that orders the elements by increasing atomic number and common properties. The atomic number is the number of protons in every atom of the element.

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    Find step-by-step solutions and answers to Chemistry - 9780130543844, as well as thousands of textbooks so you can move forward with confidence. ... Chemical Periodicity. Section 14.1: Classification of the Elements. Section 14.2: Periodic Trends. Page 409: Chapter Review. Page 411: Standardized Test Prep. Exercise 1a. Exercise 1b. Exercise 1c ...

  20. S-C-5-3 Periodic Trends Worksheet and KEY

    ANSWER KEY Periodic Trends Worksheet 1. Using the data below, make a bar graph of atomic radius vs. atomic number for Group 2A and for Period 3 of the periodic table. Group 2A Element Atomic Number Atomic Radius Be 4 1. Mg 12 1. Ca 20 1. Sr 38 2. Ba 56 2. 2. What trends do you notice for the atomic radii of Group 2A?

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  23. Periodic Trends Answer Key

    CHM 252 Syllabus Spring 2023. The Periodic Table of the Elements. Worksheets. General Chemistry 1 Worksheets. General Chemistry 2 Worksheets. Activation Energy. Activation Energy Answer Key. Calculation of Kc and Kp. Calculation of Kc and Kp Answer Key.