Question 1

Which of the following is an acidic oxide?

Accepted Answer

A)  P4O10
B)  MgO
C)  Fe2O3
D)  K2O
E)  Cr2O3

Question 2

The general electron configuration for atoms of the halogen group is

Accepted Answer

A)  ns2np6.
B)  ns2np5.
C)  ns2np6(n -1) d7.
D)  ns1.
E)  ns2np7.

Question 3

The sulfide ion, S2-,  is isoelectronic with which one of the following?

Accepted Answer

A)  O2-
B)  F-
C)  Na+
D)  Al3+
E)  K+

Question 4

Which two electron configurations represent elements that would have similar chemical properties? (1) 1s22s22p4 (2) 1s22s22p5 (3) [Ar]4s23d5 (4) [Ar]4s23d104p5

Accepted Answer

A)  (1) and (2) 
B)  (1) and (3) 
C)  (2) and (3) 
D)  (2) and (4) 
E)  (3) and (4)

Question 5

How many electrons are in the 4p orbitals of vanadium?

Accepted Answer

A)  0
B)  2
C)  4
D)  5
E)  6

Question 6

Consider the following reaction 2A + 3F2  →\rarr→ 2AF3. What is the formula for the reaction product if we substitute sulfur for fluorine?

Accepted Answer

A)  A2S3
B)  A3S2
C)  AS3
D)  A3S
E)  AS

Question 7

Which one of the following does not have [Kr] as its electronic configuration?

Accepted Answer

A)  Se2-
B)  Br-
C)  Rb+
D)  Y3+
E)  Zn2+

Question 8

Which of the following is a basic oxide?

Accepted Answer

A)  CO2
B)  MgO
C)  As2O3
D)  SO2
E)  Cl2O7

Question 9

Which of the following ground-state ions has the largest number of unpaired electrons?

Accepted Answer

A)  Cr2+
B)  Mn2+
C)  Ni2+
D)  Cu+
E)  Co2+

Question 10

Write the ground-state electron configuration for Al3+.

Accepted Answer

Question 11

How many valence electrons does a tin (Sn) atom have?

Accepted Answer

A)  2
B)  4
C)  14
D)  36
E)  50

Question 12

Which pair of elements from different groups resemble each other the most in their chemical properties?

Accepted Answer

A)  Be and B
B)  Al and Si
C)  Li and Be
D)  Al and Be
E)  Be and C

Question 13

Which of the following elements has the greatest metallic character?

Accepted Answer

A)  Br
B)  Se
C)  Ni
D)  As
E)  Si

Question 14

Given the following melting point data, what is a reasonable estimate of the melting point of potassium?

Accepted Answer

The answer of Given the following melting point data, what...

Question 15

For silicon atoms, which ionization energy will show an exceptionally large increase over the preceding ionization energy?

Accepted Answer

A)  2nd
B)  3rd
C)  4th
D)  5th
E)  6th

Question 16

Write the ground-state electron configuration for Br-.

Accepted Answer

Question 17

The successive ionization energies of a certain element are I1 = 577.9 kJ/mol, I2 = 1820 kJ/mol, I3= 2750 kJ/mol, I4 = 11,600 kJ/mol, and I5 = 14,800 kJ/mol. This pattern of ionization energies suggests that the unknown element is

Accepted Answer

A)  K.
B)  Al.
C)  Cl.
D)  Se.
E)  Kr.

Question 18

Which of the elements listed below has the highest first ionization energy?

Accepted Answer

A)  He
B)  Ne
C)  Ar
D)  Kr
E)  Xe

Question 19

The first ionization energy of sodium is 495.9 kJ/mol. The energy change for the reaction Na(s)  →\rarr→  Na+(g) + e- is therefore

Accepted Answer

A)  495.9 kJ/mol.
B)  less than 495.9 kJ/mol.
C)  greater than 495.9 kJ/mol.
D)  is equal to the electron affinity of sodium.
E)  is equal to the second ionization energy of sodium.

Question 20

Which of the following elements behaves chemically similarly to potassium?

Accepted Answer

A)  magnesium
B)  sodium
C)  beryllium
D)  chlorine
E)  iron

Exam 8: The Periodic Table

For silicon atoms, which ionization energy will show an exceptionally large increase over the preceding ionization energy?

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The sulfide ion, S2-, is isoelectronic with which one of the following?

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The general electron configuration for atoms of the halogen group is

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How many valence electrons does a tin (Sn) atom have?

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Which of the following is a basic oxide?

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The successive ionization energies of a certain element are I1 = 577.9 kJ/mol, I2 = 1820 kJ/mol, I3= 2750 kJ/mol, I4 = 11,600 kJ/mol, and I5 = 14,800 kJ/mol. This pattern of ionization energies suggests that the unknown element is

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Which of the following elements has the greatest metallic character?

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Which one of the following does not have [Kr] as its electronic configuration?

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The first ionization energy of sodium is 495.9 kJ/mol. The energy change for the reaction Na(s) →\rarr→ Na+(g) + e- is therefore

Correct AnswerverifiedShow Answer

Consider the following reaction 2A + 3F2 →\rarr→ 2AF3. What is the formula for the reaction product if we substitute sulfur for fluorine?

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Which of the elements listed below has the highest first ionization energy?

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Which of the following elements behaves chemically similarly to potassium?

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Which two electron configurations represent elements that would have similar chemical properties? (1) 1s22s22p4 (2) 1s22s22p5 (3) [Ar]4s23d5 (4) [Ar]4s23d104p5

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Which pair of elements from different groups resemble each other the most in their chemical properties?

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Write the ground-state electron configuration for Al3+.

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Given the following melting point data, what is a reasonable estimate of the melting point of potassium?

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Which of the following ground-state ions has the largest number of unpaired electrons?

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How many electrons are in the 4p orbitals of vanadium?

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Which of the following is an acidic oxide?

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Write the ground-state electron configuration for Br-.

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The sulfide ion, S^2-, is isoelectronic with which one of the following?

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The successive ionization energies of a certain element are I₁= 577.9 kJ/mol, I₂= 1820 kJ/mol, I₃= 2750 kJ/mol, I₄ = 11,600 kJ/mol, and I₅ = 14,800 kJ/mol. This pattern of ionization energies suggests that the unknown element is

Correct Answer
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The first ionization energy of sodium is 495.9 kJ/mol. The energy change for the reaction Na(s) $\rarr$ Na⁺(g) + e^- is therefore

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Consider the following reaction 2A + 3F₂ $\rarr$ 2AF₃. What is the formula for the reaction product if we substitute sulfur for fluorine?

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Which two electron configurations represent elements that would have similar chemical properties? (1) 1s²2s²2p⁴ (2) 1s²2s²2p⁵ (3) [Ar]4s²3d⁵ (4) [Ar]4s²3d¹⁰4p⁵

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Write the ground-state electron configuration for Al³⁺.

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Write the ground-state electron configuration for Br^-.

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