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1.7 Periodic Trends

8 min read β€’ december 21, 2022

Dalia Savy

Jeremy Kiggundu

A cool thing about the periodic table is that it is organized to demonstrate different trends and properties of elements that can be explained by the pattern of electron configurations and the presence of electron-filled orbitals.Β The periodicity of the periodic table , or its tendency to recur at intervals, can help you estimate the properties of atoms that haven't even been discovered yet.

For the sake of the AP Chemistry exam, rather than only understanding the trends, you should be able to explain why they happen.

Foundational Concepts for Periodic Trends

In order to fully understand why the trends occur the way they do, it's important to cover the following topics:

Organization of the Periodic Table

As mentioned before, the periodic trends aren't too difficult to grasp since they follow the chronology of the periodic table . It was purposely made to group chemicals of similar properties together.

It is also important to note that the periodic table is divided into 18 columns (called groups ) and 7 rows (called periods ).

Periods on the Periodic Table

🀨 Properties that differ: Going horizontally, each period is organized in order of increasing atomic number . The atomic number , or the number of protons in an atom's nucleus, determines the basic chemical properties of said element. This trend contributes to the differing effective nuclear charge of elements in the same group, which we'll discuss below.

🀝 Shared Properties: In each row, the elements have the same number of occupied electron shells .

Let's compare sodium, which is the first element in period 3, with argon, the last element in period 3.

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You could see here that both sodium and argon have a total of three occupied electron shells , following the pattern of elements in the same period. However, sodium has 11 protons (represented by its atomic number of 11), and argon has 18 protons (represented by its atomic number of 18).

Groups on the Periodic Table

🀨 Properties that differ: One group on the periodic table is organized so that as you move down a group, the number of occupied electron shells increase.

🀝 Shared Properties: Every element in one group has the same number of valence electrons in its outermost shell. Because these elements all have the same number of valence electrons , they can bond to other elements in similar ways. In other words, these elements tend to have similar chemical properties.

Some groups on the periodic table have a name, since the elements in a single group have similar properties. For example, the elements in group 18 are called noble gases . All noble gases are generally unreactive due to their high stability.

Let's now compare neon, the second noble gas in group 18, with xenon, the fifth noble gas.

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Both neon and xenon have eight valence electrons in their outermost shell, but neon only has two occupied electron shells , while xenon has five occupied electron shells . The fact that they both have a full octet, or eight valence electrons in their outermost shell, makes them both noble gases . Having a full octet makes these elements very stable, and therefore unreactive.

Effective Nuclear Charge

What two subatomic particles make up the nucleus? Protons and neutrons, right? Since neutrons are neutral, protons are the particles that contribute to the positive charge of the nucleus, or the actual nuclear charge (Z).

Now, try to connect this to Coulomb's law which calculates the attraction between two atoms. Each electron orbiting the nucleus experiences both an attraction to the nucleus and a repulsion from the atom's other electrons.

Electrons that are in the outer shells of an atom may be shielded by the innermost electrons because of the electron-electron repulsion present. In order to accurately represent the nuclear charge of a nucleus, we must account for both the actual nuclear charge and the charge shielded by other electrons (S).

You do not need to know this formula for the AP exam, but it may help you better understand nuclear charge. Effective nuclear charge is equal to the actual nuclear charge (Z) - the charge shielded by other electrons (S).

πŸ‘‰ Want to read more about Coulomb's law? Check out this study guide on "Atomic Structure and Electron Configuration."

5 Periodic Trends to Know for AP Chemistry

Let's try to apply the concepts above to the five periodic trends that you should learn and understand for the AP Chemistry exam. The best way to conceptualize this information is to think about it through the concepts we went over above. When in doubt, think about nuclear charge and the periodicity of the periodic table .

Atomic Radius

The atomic radius of an atom is the distance between an atom's nucleus and its valence electrons .

Across a Period - Smaller

Going from left to right on the periodic table , the atomic radii get smaller. As you go right, the atomic numbers increase. This means that there is a higher nuclear charge which increases the pull the nucleus has on the electrons. The closer the electrons are to the nucleus, the smaller the distance.

This trend can also be explained by the fact that all elements in a period have the same number of shells. For example, both Li and F have 2 shells, like Na and Ar both have 3 shells.

Down a Group - Larger

As you go down a group on the periodic table , the atomic radii increase. This is because the number of occupied shells increases. For example in group 1, Li has 2 occupied shells while Cs has 6 occupied electron shells (similar to the trend explained above with neon and xenon).

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Image Courtesy of Thivyaapriya

Ionic Radius

The ionic radius is the distance between the nucleus of an ion and the valence electrons of that said ion.

When metals ionize, they lose an electron and become positive ions. Losing an electron makes the ion decrease in size. There is also less shielding and electron-electron repulsion present, allowing the remaining valence electrons to be closer to the nucleus.

Sometimes, metals lose their entire valence shell, significantly decreasing their size.

When nonmetals ionize, they gain an electron and become negative ions. Gaining an electron makes the ion increase in size. There is also more electron-electron repulsion present due to the increased number of negatively charged particles.

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Electronegativity

Electronegativity refers to how strongly a nucleus attracts electrons of another atom.

Across a Period - Increases

This is because the elements on the right side of the periodic table (such as noble gases in group 18) have more protons in their nuclei, which gives them a greater positive charge. Having a greater nuclear charge makes the nuclei more effective at attracting electrons.

Down a Group - Decreases

As you go down a group, the atomic size of an atom increases. Therefore, the nucleus of one atom is farther away from the electrons of another atom, and the attraction between the two is weaker.

Ionization Energy

Ionization energy is the amount of energy needed to remove the valence electrons of an atom. Since there are often multiple valence electrons , there are multiple ionization energies. The first I.E. is the amount required to remove the most loosely held electron and the second I.E. is the amount required to remove the second most loosely held electron.

Since size decreases across a period, the nucleus and the electrons are more closely attracted to each other. This stronger attraction makes it harder to remove a valence electron. Thus, it takes more energy to do so.

As you go down a group, the amount of occupied electron shells increases. The valence electrons that are farther away are more loosely attracted to the nucleus. Therefore, it takes less energy to remove them.

Information to Note

The 2nd I.E. will always be greater than the first since inner electrons are more strongly attracted to the nucleus.

There are some exceptions to this trend!

1st I.E. for group 15 > 1st I.E. for group 16.

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This highlighted electron is in an already occupied orbital. The shielding experienced will lower the required energy to remove the outermost electron, making the 1st I.E. lower than expected for S.

I.E. of Be>B and Mg>Al because of something called quantum tunneling .

Quantum Tunneling - The 2p electron in B is easier to remove than a 2s electron in Be. This is because the 2p electron spends more time away from the nucleus while the 2s electron may tunnel towards the nucleus for enough time to make it more difficult to remove.

Valence Electrons

Using the ionization energies given below, determine the number of valence electrons this element has.

When you are given this type of question, just look for the huge jump in ionization energies. This gap occurs because of how much more energy it takes to remove electrons closer to the nucleus.

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Therefore, this element has 2 valence electrons !

Electron Affinity

Electron affinity is the energy change when an electron is added to an atom in the gaseous state.

Across a Period - more negative

Down a group - more positive.

The more negative the energy, the more energy is released! Electron affinity is typically negative just because an atom releases energy when it gains an electron. However, how negative depends on this trend. You may be able to explain this trend by thinking about electronegativity .

Because of this, you may expect flourine to have the highest magnitude of electron affinity . However, chlorine does! Flourine is too small of an atom and the electrons are so close together that they would repel, which takes energy.

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πŸ‘‰ Watch Jacob Jeffries discuss and demonstrate the periodic trends, as well as go over density.

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Periodic Trends Quiz

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This online quiz is intended to give you extra practice in identifying different periodic trends such as atomic radius, ionization energy and electron affinity. This quiz aligns with the following NGSS standard(s): HS-PS1-1 , HS-PS1-2

Select your preferences below and click 'Start' to give it a try!

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Periodic Table Trends

This chapter revisits the periodic table, this time focusing more on some specific properties of the elements that change in a predictable way. Students will learn about electronegativity, electron affinity, atomic radius, and ionization energy.

Periodic Table History and Trends Lecture

Purpose:  This is a Powerpoint lecture that briefly covers the discovery of the periodic table by Demitri Mendeleev, defines the different groupings of the periodic table, then explains some of the important trends seen within the atoms.

Essential Concepts: Periodic table, period, family, group, alkali metals, alkaline earth metals, transition metals, metals, metallic character, malleable, ductile, conducrtive, alloy, metalloid, nonmetal, halogens, noble gases, periodic trends, electronegativity, electron affinity, ionization energy, shielding.

Periodic Table History and Trends Notes Outline

Purpose:  This is a fill-in-the-blank style notes outline for students to complete as you complete the accompanying Powerpoint lecture. Each slide has a set of questions, fill-in-the-blanks, or tables that students fill in based on the information given. This is a good aid for students who struggle with taking notes freehand.

Graphing Periodic Trends

Purpose:  This is an activity meant to have students track and compare changes in electronegativity and atomic radius across a period and down a group.

Essential concepts: Periodic trends, group, period, electronegativity, atomic radius.

Periodic Table Trends Study Guide

Purpose:  Once the instruction for the unit is completed, students can complete this study guide to aid in their preparation for a written test. The study guide is divided into two sections: vocabulary and short answer questions. The vocabulary words can be found scattered throughout the different instructional worksheets from this unit. The short answer questions are conceptual and meant to see if the students are able to apply what they've learned in the unit.

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Periodic Table - Ch. 6

Worksheet - Periodic Trends Lab - Periodic Law Activity - Operation: Periodic Table Activity - What Element Am I? Activity - Periodically Puzzling

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Worksheet - Molecular Compounds Worksheet - Ionic Compounds Worksheet - Acids Lab - Ionic vs. Covalent Activity - Formula Fun!

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Trends in the Periodic Table I - Atomic and Ionic Radius (Worksheet)

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Name: ______________________________

Section: _____________________________

Student ID#:__________________________

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.

Learning Objectives

  • Predict the variation in atomic radius in the periodic table.
  • Describe specific reasons for this variation across a period and within a group.
  • Predict differences in atomic radius and ionic radius for the same element; predict differences in ionic radius for various oxidation states of the same element.

Many of the trends in the periodic table are useful tools for predicting electronic properties and chemical reactivities of various species, including transition metal complexes. The radius of transition metal ions in inorganic coordination compounds is of great importance in many biologically relevant coordination compounds.

A. Atomic Radius

Critical thinking questions:.

  • Write out the complete electron configuration for lithium, sodium, and potassium.
  • Write out the complete electron configuration for beryllium, magnesium, and calcium.
  • How do the valence electron configurations change as you go from one element to the next in question 1? How do the valence electron configurations change as you go from one element to the next in question 2? How do the complete electron configurations differ from one another for the elements in each of the above questions?
  • Predict the trend for the atomic radius for the elements in group I and group II of the periodic table.
  • Compare your predictions to the values given in model 1 below.

Model 1: Atomic radii in groups I and II of the periodic table:

1 Slater, J.C., J. Chem. Phys. , 1964, 41 , 3199.

  • Write out the complete electron configuration of titanium, and the valence electron configurations of vanadium, chromium, iron, cobalt, arsenic, and selenium. Keep in mind that the electron configuration of some atoms differs from what may be expected.
  • How do the complete and/or valence electron configurations change as you go from one element to the next in question 6?
  • Going from left to right in period 4 of the periodic table (or any other period), what do you predict the general trend to be for the atomic radius of the elements? Consider the total number of protons and electrons, as well as the valence shell that electrons are added into when going from left to right across a period in your prediction.
  • Compare your predictions to the values given in model 2 below.

Model 2: Atomic radii in period 4 of the periodic table:

  • Are there any exceptions to the general trends for the atomic radius that can be seen in these models? If so, suggest an explanation for these exceptions.

B. Ionic Radius

  • In general, will an anion have a larger or smaller ionic radius compared to the atomic radius of the neutral element that it is derived from? Justify your answer.
  • Is the same true for cations? Justify your answer.
  • Considering your answer to the previous question, use the information given in model 2 to predict the ionic radius for Fe 2+ , Fe 3+ , V 4+ , and V 5+ .
  • Compare your predicted ionic radii from the previous question to values given in the literature.
  • Order the ions listed in question 13, as well as V 2+ and V 4+ , in order of increasing size to charge ratio.
  • Discuss at least two possible effects that a different size to charge ratio of transition metal ions derived from the same element (e.g. Fe 2+ and Fe 3+ ) could have on properties, reactivities, or chemical behavior of compounds containing inorganic transition metal ions.
  • Jens-Uwe Kuhn, Santa Barbara City College
  • Jessica Martin, Northeastern State University

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COMMENTS

  1. PDF Periodic Trends Practice Questions and Key

    Created Date: 11/3/2015 3:20:46 PM

  2. Periodic trends (practice)

    Periodic trends Google Classroom You might need: Periodic table The first two ionization energies for beryllium are shown below. Be ( g) β†’ Be + ( g) + e βˆ’ Be + ( g) β†’ Be 2 + ( g) + e βˆ’ I 1 = 900 kJ/mol I 2 = 1757 kJ/mol

  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. Periodic Trends Worksheet Flashcards

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    A general chemistry Libretexts Textmap organized around the textbook. Chemistry: The Central Science. by Brown, LeMay, Bursten, Murphy, and Woodward. These are homework exercises to accompany the Textmap created for "Chemistry: The Central Science" by Brown et al. Complementary General Chemistry question banks can be found for other Textmaps ...

  6. AP Chem Unit 1.7 Periodic Trends

    . The atomic number , or the number of protons in an atom's nucleus, determines the basic chemical properties of said element. This trend contributes to the differing effective nuclear charge of elements in the same group, which we'll discuss below. 🀝 Shared Properties: In each row, the elements have the same number of occupied

  7. Periodic Trends

    This means that the nucleus attracts the electrons more strongly, pulling the atom's shell closer to the nucleus. The valence electrons are held closer towards the nucleus of the atom. As a result, the atomic radius decreases. Figure 6 6: Periodic Table showing Atomic Radius Trend. Down a group, atomic radius increases.

  8. PDF Chemistry Learner

    Periodic Trends Practice Worksheet Answers Identify each element as a metal, metalloid, or nonmetal (3} (4} (5) (8, @ germanium metalloid @ phosphorous nonmetal b zinc metal @ lithium metal Which of the two species is larger in each of the following pairs?

  9. Periodic Trends Quiz : ChemQuiz.net

    This online quiz is intended to give you extra practice in identifying different periodic trends such as atomic radius, ionization energy and electron affinity. This quiz aligns with the following NGSS standard (s): HS-PS1-1, HS-PS1-2 Select your preferences below and click 'Start' to give it a try!

  10. PDF PSI AP Chemistry Name Periodic Trends MC Review

    the periodic table. 35. _____ Why atomic radius increases down a group on the periodic table. 36. _____ Why gallium has an unexpected smaller radius than aluminum? 37. _____ Why magnesium has an unexpectedly higher ionization energy that aluminum. Use the PES spectrum of Nitrogen and Oxygen below to answer questions 38-40.

  11. PDF Periodic Trends Multiple Choice Review PSI Chemistry Name

    Periodic Trends Multiple Choice Review PSI Chemistry Name_____ Atomic Size 1) Elements Z and X are compared. Element Z is larger than Element X. Based on this you could say: A) Element Z is further to the left side of the periodic table B) Element X is closer to the top of the periodic table C) Element Z and X are probably in the same group D ...

  12. PDF Periodic Trends Worksheet

    1. What trend in atomic radius do you see as you go down a group/family on the periodic table? 2. What causes this trend? 3. What trend in atomic radius do you see as you go across a period/row on the periodic table? 4. What causes this trend? 5. Circle the atom in each pair that has the largest atomic radius. a) Al B b) S O c) Br Cl

  13. Review of Periodic Trends

    Review of Periodic Trends. Show all questions. 1 / 30. =>. As one moves from left to right ( β†’ ) within a period across the periodic table, the ionization energy of the elements encountered tends to: ? increase. ? decrease.

  14. 1: Periodic Trends Worksheet (advanced)

    Data in Figure 1.5 1. 5 are from Inorganic Chemistry by Shriver and Atkins, 5th edition, Oxford University Press, Oxford, 2010. 1: Periodic Trends Worksheet (advanced) is shared under a CC BY-NC-SA 4.0 license and was authored, remixed, and/or curated by LibreTexts. This is an assignment worksheet. Please click the pdf icon on the page to ...

  15. Periodic Table Trends

    Purpose: This is a Powerpoint lecture that briefly covers the discovery of the periodic table by Demitri Mendeleev, defines the different groupings of the periodic table, then explains some of the important trends seen within the atoms.

  16. chemistry: periodic trends review worksheet Flashcards

    Preview. Terms in this set (19) rank the following elements by increasing atomic radius: carbon, aluminum, oxygen, potassium. O->C->Al->K. rank the following elements by increasing electronegativity: sulfur, oxygen, neon, aluminum. Ne->Al->S->O. difference between electron affinity and ionization energy. EA- measure of the energy change that ...

  17. Periodic Trends Worksheet and KEY

    Periodic Trends Worksheet Name _____ 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. 4 8 12 16 20 24 28 32 36 40 44 48 52 56 60 64 68 72 76 80

  18. Mrs. J's Chemistry Page

    Periodic Table - Ch. 6. Worksheet - Periodic Trends Lab - Periodic Law Activity - Operation: Periodic Table Activity - What Element Am I? Activity - Periodically Puzzling. Chemical Bonding - Ch. 6 & 7. Worksheet - Molecular Compounds Worksheet - Ionic Compounds Worksheet - Acids Lab - Ionic vs. Covalent Activity - Formula Fun!

  19. Trends in the Periodic Table I

    Jessica Martin, Northeastern State University. Trends in the Periodic Table I - Atomic and Ionic Radius (Worksheet) is shared under a CC BY-NC-SA 4.0 license and was authored, remixed, and/or curated by LibreTexts. Many of the trends in the periodic table are useful tools for predicting electronic properties and chemical reactivities of various ...

  20. Unit: Periodic Trends "History and the Basics" Flashcards

    Transition Metals. d block metals. Moseley. The second scientist who arranged the Periodic Table according to atomic number. Group. Vertical column. Metalloids. Has properties of both metals and nonmetals. Study with Quizlet and memorize flashcards containing terms like The Staircase, Atomic mass, Ductile and more.

  21. Periodic Trends Worksheet 1 answers

    eded to remove an electron from an atom. First ionization ener o remove a single valence electron from an atom. What is the periodic trend for first ionization ener r charge, and decreases going a) Be, Mg, Sr b) Bi, Cs, Ba c) Na, Which element in each pair has a higher electrone What is the periodic trend for electronegativit

  22. Trends in periodic table worksheet

    Periodic trends. Liveworksheets transforms your traditional printable worksheets into self-correcting interactive exercises that the students can do online and send to the teacher. ... School subject: Chemistry (1061818) Main content: Periodic Table (2009473) Periodic trends ...