10. Periodic Properties of the Elements

Periodic Trend: Atomic Radius

Atomic and Ionic Radius

Why do atomic radii decrease from left to right across a period of the periodic table?

With the exception of helium, the noble gases condense to 
form solids when they are cooled sufficiently. At temperatures 
below 83 K, argon forms a close-packed solid whose 
structure is shown below. (c) Based on this comparison would you say that the atoms 
are held together by chemical bonds in solid argon? 
<img src="https://lightcat-files.s3.amazonaws.com/problem_images/ef48cc9d444b8702-1660838079559.jpg" alt="" />

Choose the larger atom in each pair.
a. Sn or Si 
b. Br or Ga 
c. Sn or Bi 
d. Se or Sn

A portion of a two-dimensional “slab” of NaCl(s) is shown 
here (see Figure 8.2) in which the ions are numbered. 
(a) Which colored balls must represent sodium ions?
<img src="https://lightcat-files.s3.amazonaws.com/problem_images/4443bfba3edcf463-1661441784665.jpg" alt="" />

Be is smaller than Mg due mainly to differences in Zeff.

This difference is due to the size of orbitals occupied by the valence electrons.

Na is larger than Mg due mainly to differences in the principal quantum number.

This difference is due to differences in Zeff.

C is smaller than F due to an increase in the outermost energy levels of electrons.

C is larger than F due to the increase effective nuclear charge from C to F.

P is larger than N due primarily to stronger attractions between electrons in the outermost orbitals.

Ca is larger than Mg due to larger orbitals.

Correct, the valence electrons of Ca are further from the nucleus.

 Review trends in effective nuclear charge and principal quantum number on atomic size. 

Periodic Trends: Electronegativity, Ionization Energy, Atomic Radius - TUTOR HOTLINE

Which of the following pairs of elements would you expect to have the most similar atomic radii? 
a. Si and Ga 
b. Si and Ge 
c. Si and As

Periodic Trend: Atomic Radius Example 1

Using only the periodic table, arrange each set of atoms in
order of increasing radius: (b) S, Si, Sr

Increase because the nucleus is getting stronger.

Increase because electrons are being placed in higher n-values.

Decrease because the nucleus is getting stronger.

Increase because electrons are being added to degenerate orbitals.

Decrease because electrons are being placed in higher n-values.

In moving from top to bottom in the same column on the periodic table, what trend is expected for atomic size?&nbsp;

Ionic Radius

Consider the elements: Na, Mg, Al, Si, P.
b. Which element has the smallest atomic radius?

Oxygen is smaller than nitrogen and phosphorus is smaller than silicon.

Correct, the set involves both the change in size vertically and horizontally.

Cl and S are larger than F and O, respectively.

 As you move down a column in the periodic table, atomic radius increases.  As you move to the right across a period in the periodic table, atomic radius decreases. 

In which of the sets given are the atoms listed in order of increasing size (smallest to largest)?

The following observations are made about two hypothetical
elements A and B: The A¬A and B¬B bond lengths in the
elemental forms of A and B are 236 and 194 pm, respectively.
A and B react to form the binary compound AB2, which has
a linear structure (that is B-A-B = 180°). Based on these
statements, predict the separation between the two B nuclei
in a molecule of AB2.

Periodic Trends: Atomic Radius

In Table 7.8, the bonding atomic radius of neon is listed as
58 pm, whereas that for xenon is listed as 140 pm. A classmate
of yours states that the value for Xe is more realistic
than the one for Ne. Is she correct? If so, what is the basis
for her statement?

The experimental Pb¬Cl bond length in lead(II)chloride, 
PbCl2, is 244 pm. Based on this value and data in Figure 7.7, 
predict the atomic radius of Pb.<img src="https://lightcat-files.s3.amazonaws.com/problem_images/a2d25115b712e203-1660839406878.jpg" alt="" />

Using only the periodic table, arrange each set of atoms in
order from largest to smallest: (c) C, Cl, Cu.

Order the following atoms according to increasing atomic radius: Rb, Cl, As, K.

Which element has the largest atomic radius? (LO 5.20) 
(a) Rb 
(b) Co
(c) Mg
d) As

The Periodic Table EXPLAINED | Chemical Families and Periodic Trends

The elements with atomic numbers 35 and 53 have similar 
chemical properties. Based on their electronic configurations, 
predict the atomic number of a heavier element that also 
should share these chemical properties.

Order the following atoms according to increasing atomic radius: S, F, O.

Consider S, Cl, and K and their most common ions. (a) List
the atoms in order of increasing size.

Note from the following table that there is a significant increase
in atomic radius upon moving from Y to La, whereas
the radii of Zr to Hf are the same. Suggest an explanation for
this effect.
Atomic Radii (pm)
Sc 170 Ti 160
Y 190 Zr 175
La 207 Hf 175

Trends in the Periodic Table

Moving towards the top right corner of the Periodic Table causes the atomic radii to decrease.

Ionization Energy and Atomic Radius

Choose the larger atom in each pair.
a. Al or In 
b. Si or N 
c. P or Pb 
d. Si or Cl

Tungsten has the highest melting point of any metal in the
periodic table: 3422 °C. The distance between W atoms in
tungsten metal is 274 pm. (a) What is the atomic radius of
a tungsten atom in this environment? (This radius is called
the metallic radius.)

Which alkaline earth metal has the smallest atomic radius?&nbsp;

Which of the following three spheres represents a Ca atom, which an Sr atom, and which a Br atom?
<img src="https://lightcat-files.s3.amazonaws.com/problem_images/7708f68282184b2f-1669915523670.jpg" alt="" />

Which of the following statements about the bonding atomic
radii in Figure 7.7 is incorrect?
(i) For a given period, the radii of the representative elements generally decrease from left to right across a period.
(ii) The radii of the representative elements for the n = 3 period are all larger than those of the corresponding elements in the n = 2 period.
(iii) For most of the representative elements, the change in radius from the n = 2 to the n = 3 period is greater than the change in radius from n = 3 to n = 4.
(iv) The radii of the transition elements generally increase moving from left to right within a period.
(v) The large radii of the Group 1 elements are due to their relatively small effective nuclear charges.<img src="https://lightcat-files.s3.amazonaws.com/problem_images/f1776405d4e660ac-1660839574013.jpg" alt="" />

The Periodic Table: Atomic Radius, Ionization Energy, and Electronegativity

Which atom in each of the following pairs has a larger radius?
(a) Na or K
(b) V or Ta
(c) V or Zn
(d) Li or Ba

Which atom in each of the following pairs has a larger radius?
(a) C or Ge
(b) Ni or Pt
(c) Sn or I
(d) Na or Rb

Which quantity must be determined experimentally in
order to determine the bonding atomic radius of an atom?
(a) The distance from the nucleus where the probability of finding an electron goes to zero.
(b) The distance between the nuclei of two atoms that are bonded together.
(c) The effective nuclear charge of an atom.

Arrange the following atoms in order of decreasing atomic radius:Sr, Se, Ne, Zn

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1. Intro to General Chemistry

2. Atoms & Elements

3. Chemical Reactions

4. BONUS: Lab Techniques and Procedures

5. BONUS: Mathematical Operations and Functions

6. Chemical Quantities & Aqueous Reactions

7. Gases

8. Thermochemistry

9. Quantum Mechanics

11. Bonding & Molecular Structure

12. Molecular Shapes & Valence Bond Theory

13. Liquids, Solids & Intermolecular Forces

14. Solutions

15. Chemical Kinetics

16. Chemical Equilibrium

17. Acid and Base Equilibrium

18. Aqueous Equilibrium

19. Chemical Thermodynamics

20. Electrochemistry

21. Nuclear Chemistry

22. Organic Chemistry

23. Chemistry of the Nonmetals

24. Transition Metals and Coordination Compounds

[BOOK CHEM] Clutch Version

Periodic Trend: Cumulative

Periodic Trends are patterns present in the periodic table based on an element's size and electron distribution.&nbsp;

Periodic Trend: Ionic Radius

Ionic Radius is the distance between an ion's nucleus and its most outer occupied electron shell.&nbsp;

The Electron Configuration

The electron configuration of an element is the distribution of its electrons within atomic orbitals.&nbsp;

The Electron Configuration: Ions

The Electron Configuration of Ions involves either adding or removing electrons from a given orbital of an element.

Periodic Trend: Successive Ionization Energies

Successive Ionization Energies deals with the removal of multiple electrons from a gaseous atom or ion through multiple steps.

The atomic radius of an element is the distance from its nucleus to its outer electron shell.

Valence Electrons of Elements

The Valence Electrons represent the outer shell electrons of an element or ion.&nbsp;

Periodic Trend: Effective Nuclear Charge

Effective Nuclear Charge (Zeff) measures the force exerted onto an electron by the nucleus.&nbsp;

Periodic Trend: Ionization Energy

Ionization Energy is the energy absorbed&nbsp;in order to remove an electron from a gaseous atom or ion.&nbsp;

Periodic Trend: Metallic Character

Metallic Character&nbsp;deals with how easily an electron can be removed from an element.&nbsp;

Paramagnetism and Diamagnetism

Paramagnetism&nbsp;and&nbsp;Diamagnetism deal with the presence of electrons that are either unpaired or paired in an orbital.

Periodic Trend: Electron Affinity

Electron Affinity is the energy released from the addition of an electron to a gaseous atom or ion.&nbsp;

The Electron Configuration: Quantum Numbers

The Quantum Numbers ultimately can be used to determine the precise location of an electron.&nbsp;

Periodic Trend: Electronegativity

Electronegativity is an element's ability to attract electrons.

The Electron Configurations: Exceptions

Most Electron Configuration Exceptions are the result of elements drive to obtain half filled or totally filled d orbitals.&nbsp;

The Electron Configuration: Condensed

Condensed Electron Configurations are a faster method in determining the configuration of elements and ions.&nbsp;