Question 1

The most basic oxides are formed from elements found in the __________ region of the periodic table.

Accepted Answer

A) upper right 
B) upper left 
C) center 
D) lower right 
E) lower left

Question 2

Which of the following elements has the smallest atomic size?

Accepted Answer

A) Na 
B) Ar 
C) K 
D) Ca 
E) Kr

Question 3

Select the most acidic compound from the following.

Accepted Answer

A) SO 2 
B) Al 2O 3 
C) CaO 
D) PbO 
E) H 2O

Question 4

Select the correct electron configuration for sulfur (Z = 16).

Accepted Answer

A) 1 s 21 p 62 s 22 p 6 
B) 1 s 22 s 22 p 83 s 23 p 4 
C) 1 s 22 s 22 p 83 s 23 p 2 
D) 1 s 22 s 22 p 63 s 23 p 4 
E) 1 s 22 s 22 p 63 s 23 d 4

Question 5

The effective nuclear charge for an atom is less than the actual nuclear charge due to

Accepted Answer

A) shielding. 
B) penetration. 
C) paramagnetism. 
D) electron-pair repulsion. 
E) relativity.

Question 6

In moving down a group in the periodic table, the oxides of the elements become more acidic in nature.

Accepted Answer

A) True 
 B)False

Question 7

Which of the following electron configurations is correct for the excited state of an element?

Accepted Answer

A) [He]2 s 22 p 5 
B) [Ne]3 s 23 p 1 
C) [Ar]4 s 14 p 1 
D) [Kr]5 s 24 d 7 
E) [He]1 p 1

Question 8

In the ground state of an atom of silver (Ag), how many electrons will there be with the quantum number l = 1? (The n, ml, and ms quantum numbers may have any appropriate values.)

Accepted Answer

A) 9 
B) 12 
C) 18 
D) 24 
E) 36

Question 9

In Mendeleev's version of the periodic table, the elements were arranged in order of increasing atomic number.

Accepted Answer

A) True 
 B)False

Question 10

How many valence electrons are there in an atom with the electron configuration [noble gas]ns2(n −1)d10np3?

Accepted Answer

A) 2 
B) 3 
C) 5 
D) 10 
E) 15

Question 11

Which of the following electron configurations is impossible?

Accepted Answer

A) 1 s 22 s 22 p 63 s 23 p 4 
B) 1 s 22 s 22 p 53 s 13 p 4 
C) 1 s 22 s 22p 63 s 23 p 63 d 104 s 2 
D) 1 s 22 s 22 p 63 s 33 p 4 
E) 1 s 12 s 22 p 63 s 23 p 4

Question 12

The electronic structure 1s22s22p63s23p64s23d8 refers to the ground state of

Accepted Answer

A) Kr. 
B) Ni. 
C) Fe. 
D) Pd. 
E) None of these choices are correct.

Question 13

Which one of the following equations correctly represents the process involved in the electron affinity of X?

Accepted Answer

A) X( g)→ X +( g)+ e − 
B) X +( g)→ X +( aq) 
C) X +( g)+ e − → X( g) 
D) X( g)+ e − → X −( g) 
E) X +( g)+ Y −( g)→ XY( s)

Question 14

Which of the following elements has the largest atomic size?

Accepted Answer

A) S 
B) Ca 
C) Ba 
D) Po 
E) Rn

Question 15

In many-electron atoms, which quantum numbers specify the energy of an electron?

Accepted Answer

A) n and l 
B) n and ml 
C) l and ml 
D) n and ms 
E) n, l, and ml

Question 16

In neutral atoms, the 3d orbitals have higher energy than the 4s orbitals.

Accepted Answer

A) True 
 B)False

Question 17

Bigger atoms generally have smaller ionization energies.

Accepted Answer

A) True 
 B)False

Question 18

First ionization energies of neutral atoms may be positive or negative.

Accepted Answer

A) True 
 B)False

Question 19

An atom of element number 33 (As) is in its ground electronic state. Which one of the following sets quantum numbers could not apply to any of its electrons?

Accepted Answer

A) n = 2 l = 1 ml = −1 ms = +½ 
B) n = 3 l = 0 ml = 0 ms = −½ 
C) n = 3 l = 2 ml = −2 ms = −½ 
D) n = 4 l = 0 ml = 0 ms = −½ 
E) n = 4 l = 2 ml = 1 ms = +½

Question 20

Which of the following atoms will be diamagnetic?

Accepted Answer

A) Cr 
B) Ru 
C) Fe 
D) Pt 
E) Cd

Exam 8: Electron Configuration and Chemical Periodicity

The most basic oxides are formed from elements found in the __________ region of the periodic table.

Which of the following elements has the smallest atomic size?

Select the most acidic compound from the following.

Select the correct electron configuration for sulfur (Z = 16) .

The effective nuclear charge for an atom is less than the actual nuclear charge due to

In moving down a group in the periodic table, the oxides of the elements become more acidic in nature.

Which of the following electron configurations is correct for the excited state of an element?

In the ground state of an atom of silver (Ag) , how many electrons will there be with the quantum number l = 1? (The n, m_l, and m_s quantum numbers may have any appropriate values.)

In Mendeleev's version of the periodic table, the elements were arranged in order of increasing atomic number.

How many valence electrons are there in an atom with the electron configuration [noble gas]ns²(n −1) d¹⁰np³?

Which of the following electron configurations is impossible?

The electronic structure 1s²2s²2p⁶3s²3p⁶4s²3d⁸refers to the ground state of

Which one of the following equations correctly represents the process involved in the electron affinity of X?

Which of the following elements has the largest atomic size?

In many-electron atoms, which quantum numbers specify the energy of an electron?

In neutral atoms, the 3d orbitals have higher energy than the 4s orbitals.

Bigger atoms generally have smaller ionization energies.

First ionization energies of neutral atoms may be positive or negative.

An atom of element number 33 (As) is in its ground electronic state. Which one of the following sets quantum numbers could not apply to any of its electrons?

Which of the following atoms will be diamagnetic?

Exam 8: Electron Configuration and Chemical Periodicity

The most basic oxides are formed from elements found in the __________ region of the periodic table.

Which of the following elements has the smallest atomic size?

Select the most acidic compound from the following.

Select the correct electron configuration for sulfur (Z = 16) .

The effective nuclear charge for an atom is less than the actual nuclear charge due to

In moving down a group in the periodic table, the oxides of the elements become more acidic in nature.

Which of the following electron configurations is correct for the excited state of an element?

In the ground state of an atom of silver (Ag) , how many electrons will there be with the quantum number l = 1? (The n, ml, and ms quantum numbers may have any appropriate values.)

In Mendeleev's version of the periodic table, the elements were arranged in order of increasing atomic number.

How many valence electrons are there in an atom with the electron configuration [noble gas]ns2(n −1) d10np3?

Which of the following electron configurations is impossible?

The electronic structure 1s22s22p63s23p64s23d8 refers to the ground state of

Which one of the following equations correctly represents the process involved in the electron affinity of X?

Which of the following elements has the largest atomic size?

In many-electron atoms, which quantum numbers specify the energy of an electron?

In neutral atoms, the 3d orbitals have higher energy than the 4s orbitals.

Bigger atoms generally have smaller ionization energies.

First ionization energies of neutral atoms may be positive or negative.

An atom of element number 33 (As) is in its ground electronic state. Which one of the following sets quantum numbers could not apply to any of its electrons?

Which of the following atoms will be diamagnetic?

In the ground state of an atom of silver (Ag) , how many electrons will there be with the quantum number l = 1? (The n, m_l, and m_s quantum numbers may have any appropriate values.)

How many valence electrons are there in an atom with the electron configuration [noble gas]ns²(n −1) d¹⁰np³?

The electronic structure 1s²2s²2p⁶3s²3p⁶4s²3d⁸refers to the ground state of