Chemistry Chapter 7

Order the following atoms from largest to smallest atomic radius: N, O, Mg, Si, P

Mg > Si > P > N > O

For which of the following atoms are electron(s) in the 3s orbital furthest from the nucleus? a. K b. Ca c. Rb d. Sr e. they are all the same distance from the nucleus

a

For which of the following atoms are the n=1 shell electrons furthest from the nucleus? a. O b. S c. Se d. Te

a

Which of the following would you predict would have the most negative electron affinity? a. Cl b. Ar c. Se d. Na e. K

a

For which of the following atoms are electron(s) in the 3s orbital closest to the nucleus? a. Na b. Mg c. Al d. Si e. they are all the same distance from the nucleus

d

Which of the following atoms will have the largest first-ionization energy? a. Na b. Al c. Se d. Cl e. I

d

Which of the following would you predict would have the most negative electron affinity? a. Na b. Li c. Be d. S e. Ar

d

When determining the effective nuclear charge of an electron in an atom in a row of the periodic table using the simple rule Zeff = Z - S, what assumptions must be made? a. (a) all electrons of a given "n" value are treated identically b. (b) electrons with the same "n" value do not shield one another significantly c. (c) electrons in energy levels higher than the energy level of the electron of interest provide shielding d. (d) both assumptions (a) and (b) are made e. all of the above assumptions are made

d.

An electron in which of the following orbitals will be shielded most effectively from the nuclear charge? a. 1s b. 2s c. 2p d. 3s e. 3p

e

For which of the following atoms are the n=1 shell electrons closest to the nucleus? a. O b. N c. S d. As e. Se

e

The electrons in which subshell of tin (Sn) will feel the least effective nuclear charge? a. 2s b. 2p c. 4d d. 5s e. 5p

e

Which of the following atoms will have the lowest first-ionization energy? a. Li b. B c. F d. Cl e. Na

e

Which of the following statements correctly summarizes the general trends observed (with a couple notable exceptions) for electron affinity for s and p block elements in the periodic table (excluding the Noble gases)? a. Electron affinity tends to become more negative when moving from top to bottom in a group, and from left to right in a row. b. Electron affinity tends to become more negative when moving from top to bottom in a group, and from right to left in a row. c. Electron affinity tends to become more negative when moving from bottom to top in a group, and from left to right in a row. d. Electron affinity tends to become more negative when moving from bottom to top in a group, and from right to left in a row. e. Electron affinity tends to become more negative when moving from left to right in a row, while there is no general trend when moving up and down with a group

e

Electron affinity

the energy change associated with the addition of an electron to a gaseous atom or ion

Ionization energy

the minimum energy required to remove an electron from the ground state of the isolated gaseous atom

Electron configuration

the order of filling of orbitals; tells us which orbitals are filled or partially filled

The general trends observed for how electron affinity changes within a period (with a couple notable exceptions) can be to some degree explained by ______(i)________. The general trends observed for how electron affinity changes within a group can be explained by ______(i)________.

(i) effective nuclear charge felt by the ionizable electron; (ii) principal quantum number of, and electron-electron repulsion within the valence shell

In order to ionize an electron from gaseous sodium ___(i)____ light is required. In order to ionize an electron from gaseous sodium ___(ii)____ light is required. It takes more energy to ionize ____(iii)______ sodium.

(i) ultraviolet; (ii) blue visible; (iii) gaseous

It turns out that it requires 275 kJ/mol of energy to ionize a sodium atom present in solid sodium metal. What is the longest wavelength of electromagnetic radiation capable of ionizing sodium atoms in the solid state?

4.35 x 10⁻⁷ m

Use a simplified model for electronic structure where all electrons of a given "n" value are assumed to have the same average energies and to reside the same distance from the nucleus in answering this question: What is the effective nuclear charge (Zeff) felt by the valence electrons of Cl?

7

Use the simplified model for electronic structure where all electrons of a given "n" value are assumed to have the same average energies and to reside the same distance from the nucleus in answering this question: What would be the effective nuclear charges felt by the electrons in the (i) n = 1, (ii) n = 2, and (iii) n = 3 shells of the phosphorus (P) atom?

15, 13, and 5

(Associating principles from electronic structure with periodic properties). The ionization energy for an isolated gaseous atom of sodium is 496 kJ/mol. What is the longest wavelength of electromagnetic radiation capable of ionizing sodium atoms in the gaseous state?

2.41 x 10⁻⁷ m

Based on your knowledge of the relative energies of electrons in subshells in multielectron atoms, electron(s) in which subshell will feel the greatest effective nuclear charge?

2s

Order the following atoms from largest to smallest atomic radius: N, K, As, Fr

Fr > K > As > N

Order the following atoms from lowest to highest first-ionization energy: Cl, S, Se, Sb

Sb <Se < S < Cl

A slight decrease in first ionization energy upon going from N to O can be attributed to what factor? a. electron pairing within an orbital b. electron-nuclear distance c. electron-electron repulsion between core and valence electrons d. effective nuclear charge e. shielding of p orbitals by electrons in an s orbital with the same principle quantum number

a

Which of the following atoms is most likely to violate the general trend observed for electron affinity when moving from left to right within row 3 of the periodic table? a. Mg and S b. Mg and P c. Al and S d. Al and P e. P and S

b

Which of the following elements will have the lowest second-ionization energy? a. Cs b. Ba c. Be d. B e. Br

b

Which of the following statements correctly summarizes the general trends observed for atomic radii of the elements in the periodic table? a. Atomic radii tend to increase when moving from top to bottom in a group, and from left to right in a row. b. Atomic radii tend to increase when moving from top to bottom in a group, and from right to left in a row. c. Atomic radii tend to increase when moving from bottom to top in a group, and from left to right in a row. d. Atomic radii tend to increase when moving from bottom to top in a group, and from right to left in a row. e. Atomic radii tend to increase when moving from top to bottom in a group, but there is no significant change when moving across a row.

b

The general trends observed for how atomic radii change within a group can be explained by ______(i)________. The general trends observed for how atomic radii change within a period can be explained by ______(i)________. a. (i) principal quantum number of the ionizable electron; (ii) population of different subshells within an energy level b. (i) population of different subshells within an energy level; (ii) principal quantum number of the ionizable electron c. (i) principal quantum number of the ionizable electron; (ii) effective nuclear charge felt by the ionizable electron d. (i) effective nuclear charge felt by the ionizable electron; (ii) principal quantum number of the ionizable electron e. (i) population of different subshells within an energy level; (ii) effective nuclear charge felt by the ionizable electron

c

The general trends observed for how first ionization energies change within a group can be explained by ______(i)________. The general trends observed for how first ionization energies change within a period can be explained by ______(i)________. a. (i) principal quantum number of the ionizable electron; (ii) population of different subshells within an energy level b. (i) population of different subshells within an energy level; (ii) principal quantum number of the ionizable electron c. (i) principal quantum number of the ionizable electron; (ii) effective nuclear charge felt by the ionizable electron d. (i) effective nuclear charge felt by the ionizable electron; (ii) principal quantum number of the ionizable electron e. (i) population of different subshells within an energy level; (ii) effective nuclear charge felt by the ionizable electron

c

Three elements in n = 2 have positive electron affinities. Predict which elements they are based on your knowledge of electronic properties. a. Li, Be, B b. Li, B, O c. Be, N, Ne d. B, O, Ne e. Be, O, Ne

c

Which of the following atom would you predict to have a fourth-ionization energy very much greater than the third? a. Na b. Mg c. Al d. Si e. P

c

Which of the following atoms is most likely to violate the general trend observed for ionization energy when moving from left to right within row 3 of the periodic table? a. Mg and S b. Mg and P c. Al and S d. Al and P e. P and S

c

Which of the following atoms would you predict to have the second largest atomic radius? a. Ne b. O c. Si d. S e. Al

c

Which of the following statements correctly summarizes the general trends observed for the first ionization energy for elements in the periodic table? a. First ionization energy tends to increase when moving from top to bottom in a group, and from left to right in a row. b. First ionization energy tends to increase when moving from top to bottom in a group, and from right to left in a row. c. First ionization energy tends to increase when moving from bottom to top in a group, and from left to right in a row. d. First ionization energy tends to increase when moving from bottom to top in a group, and from right to left in a row. e. First ionization energy tends to increase when moving across a row, but there is no significant change when moving within a group.

c

Atomic radius

the typical distance from the nucleus to a boundary of the surrounding electron cloud

Valence electrons

those beyond the filled shells "outer shell electrons"

Core electrons

those in filled shells "inner shell electrons"