Deck 1: A Review of General Chemistry: Electrons, Bonds, and Molecular Properties

Question 1

What is the correct Lewis structure for PH₃?

A) I
B) II
C) III
D) IV
E) V

Answer 1

I

Question 2

Which of the following compounds are constitutional isomers of each other?

A) I & II
B) III & IV
C) I, II & III
D) I & IV
E) All of these

Answer 2

I, II & III

Question 3

What is the formal charge on oxygen in the following structure?

A) 2-
B) 1-
C) 2+
D) 1+
E) 0

Answer 3

1+

Question 4

What is the relationship between the following compounds?

A) They are isotopes
B) They are constitutional isomers
C) They are the same structure
D) They are composed of different elements
E) There is no relationship

Question 5

Chemical reactions occur as a result of:

A) Attraction between opposite charges
B) Nucleus-Nucleus interactions
C) Motion of electrons
D) Like atoms interacting
E) Combining two chemicals

Question 6

What is the correct Lewis dot structure for C?

A) I
B) II
C) III
D) IV
E) V

Question 7

Which of the following compounds are constitutional isomers of each other?

A) I & II
B) III & IV
C) I, II & III
D) II, III & IV
E) All of these

Question 8

Constitutional isomers may not differ in what aspects?

A) Physical properties
B) Atomic connectivity
C) Molecular formula
D) Name
E) Constitution

Question 9

Carbon generally forms four bonds and is considered:

A) Tetravalent
B) Divalent
C) Trivalent
D) Monovalent
E) Qudravalent

Question 10

Which of the following compounds are constitutional isomers of each other?

A) I & II
B) III & IV
C) II & III
D) I & IV
E) All of these

Question 11

What is the correct Lewis structure for CH₃CO₂H?

A) I
B) II
C) III
D) IV
E) V

Question 12

Credit for the first synthesis of an organic compound from an inorganic precursor is generally ascribed to:

A) Berzelius
B) Arrhenius
C) Kekulé
D) Wöhler
E) Lewis

Question 13

What was long thought to be the difference between inorganic and organic compounds?

A) The number of atoms
B) The synthesis of organic compounds required a vital force
C) The molecular weight
D) Inorganic compounds exhibited a strong nuclear force
E) Inorganic compounds were composed exclusively of transition metals

Question 14

Draw three constitutional isomers that have molecular formula C₄H₈BrCl

Question 15

Draw three constitutional isomers that have molecular formula C₄H₈O.

Question 16

What is the relationship between the following compounds?

A) Resonance isomers
B) Constitutional isomers
C) Empirical isomers
D) There is no relationship

Question 17

What is the correct Lewis structure for COCl₂?

A) I
B) II
C) III
D) IV
E) V

Question 18

What is the correct Lewis dot structure for S?

A) I
B) II
C) III
D) IV
E) V

Question 19

Which of the following compounds has two lone pairs on the central atom?

A) CO₂
B) SCl₂
C) NF₃
D) CS₂
E) SO₃

Question 20

What force is not taken into account in the formation of a covalent bond?

A) Repulsion between two positively charged nuclei
B) Repulsion between electron clouds on individual atoms
C) Force of attraction between positively charged nuclei and electrons
D) Repulsion of electrons by neutrons
E) All forces listed are involved in forming a covalent bond

Question 21

What is the formal charge on nitrogen in the following structure?

A) 2-
B) 1-
C) 2+
D) 1+
E) 0

Question 22

What is the correct Lewis structure for hydrocyanic acid (HCN) including the formal charges, if any?

A) I
B) II
C) III
D) IV
E) V

Question 23

Which of the following structures have 1+ formal charge on the central atom?

A) I
B) II
C) III
D) III & V
E) IV & V

Question 24

Draw Lewis structure for ^-CH₂CN including formal charges?

Question 25

What is the formal charge on oxygen in the following structure?

A) 2+
B) 2-
C) 1+
D) 1-
E) 0

Question 26

What is the formal charge on oxygen in the following structure?

A) 0
B) 1+
C) 2+
D) 1-
E) 2-

Question 27

The bonding pattern of oxygen with a formal charge of -1 could be described as:

A) One lone pair of electrons and three single bonds
B) Two lone pairs of electrons and two single bonds
C) Three lone pairs of electrons, and one single bond
D) One lone pair of electrons, one single, and one double bond
E) Zero lone pairs, and two single and one double bond

Question 28

What is the correct Lewis structure for nitric acid (HNO₃) including the formal charges?

A) I
B) II
C) III
D) IV
E) None of these

Question 29

What is the correct Lewis structure for N₂O including the formal charges, if any?

A) I
B) II
C) III
D) IV
E) V

Question 30

What is the correct Lewis structure for hydrazoic acid (HN₃) including the formal charges, if any?

A) I
B) II
C) III
D) IV
E) V

Question 31

What is the correct Lewis structure for SCN^- including the formal charges, if any?

A) I
B) II
C) III
D) IV
E) V

Question 32

What are the formal charges on boron and fluorine in the following structure?

A) B = 1+, N = 1+
B) B = 1+, N = 1-
C) B = 1-, N = 1-
D) B = 1-, N = 1+
E) B = 1-, N = 0

Question 33

What are the formal charges on boron and oxygen in the following structure?

A) B = 1-, O = 1-
B) B = 1-, O = 1+
C) B = 1+, O = 1+
D) B = 1+, O = 1-
E) B = 1-, O = 0

Question 34

Which of the following structures have zero formal charge on carbon atom?

A) I & III
B) II & III
C) III & IV
D) I & IV
E) II & IV

Question 35

Which of the following structures have 1- formal charge on sulfur atom?

A) I
B) II
C) III
D) IV
E) V

Question 36

In ammonium ion, nitrogen has a valence of 4, and zero nonbonding electrons. What is the correct formal charge of nitrogen with 4 covalent bonds?

A) 2-
B) 2+
C) 1-
D) 1+
E) 0

Question 37

Which of the following structures have 1- formal charge on nitrogen atom?

A) I
B) II
C) III
D) IV
E) V

Question 38

Which of the following structures have 1+ formal charge on sulfur atom?

A) I
B) II
C) III
D) IV
E) V

Question 39

Which of the following structures have formal charge on at least one atom?

A) I
B) II
C) III
D) IV
E) None of these

Question 40

Draw Lewis structure for NH₂CN including formal charges, if any?

Question 41

The Cl-Cl bond is best described as___________.

A) Nonpolar covalent
B) Polar covalent
C) Ionic
D) Coordinate covalent
E) None of these

Question 42

Which of the following compounds have both polar covalent and ionic bonds?

A) NH₄Br
B) H₂O₂
C) HCN
D) H₂S
E) None of these

Question 43

Which of the following is the most electronegative element?

A) P
B) N
C) S
D) O
E) F

Question 44

The electronegativity of elements on the periodic table tends to increase_______.

A) From left to right, top to bottom
B) From right to left, bottom to top
C) From left to right, bottom to top
D) From right to left, top to bottom
E) F

Question 45

Which of the following is the least electronegative element?

A) B
B) C
C) N
D) O
E) F

Question 46

Which of the following is the correct representation of dipole for P-Cl bond?

A) I
B) II
C) III
D) IV
E) V

Question 47

Which atom has the most $\delta$ + in the following compound?

A) N
B) O
C) Br
D) H
E) C

Question 48

Which of the following is the correct representation of partial charges at the indicated atoms?

A) I = $\delta$ +; II = $\delta$ +; III = $\delta$ +
B) I = $\delta$ -; II = $\delta$ -; III = $\delta$ -
C) I = $\delta$ +; II = $\delta$ +; III = $\delta$ -
D) I = $\delta$ -; II = $\delta$ -; III = $\delta$ +
E) I = $\delta$ +; II = $\delta$ -; III = $\delta$ +

Question 49

The bond between potassium and oxygen is best described as___________.

A) Nonpolar covalent
B) Polar covalent
C) Ionic
D) Coordinate covalent
E) None of these

Question 50

Which of the following series has the correct order of elements in increasing electronegativity?

A) C < N < B < Br
B) P < N < As < F
C) Li < B < N < F
D) Cl < Cs < C < Co
E) Be < B < Ba < Br

Question 51

Which of the following is the least electronegative element?

A) P
B) N
C) Mg
D) Si
E) K

Question 52

What is the correct order of increasing electronegativity for Rb, F and O?

A) Rb < F < O
B) Rb < O < F
C) O < F < Rb
D) F < Rb < O
E) None of these

Question 53

For the following compound identify the polar covalent bonds and indicate the direction of dipole moment using $\delta$ + and $\delta$ -.

Question 54

For the following compound identify the polar covalent bonds and indicate the direction of dipole moment using $\delta$ + and $\delta$ -.

Question 55

Which of the following is the most electronegative element?

A) B
B) C
C) N
D) O
E) H

Question 56

The bond between carbon and hydrogen is best described as___________.

A) Nonpolar covalent
B) Polar covalent
C) Ionic
D) Coordinate covalent
E) None of these

Question 57

Draw Lewis structure for ozone (O_3,) including formal charges, if any?

Question 58

Which of the following statements best describes the C-Cl bond in the following compound?

A) nonpolar; no dipole
B) polar; $\delta$ + at carbon and $\delta$ - at chlorine
C) polar; $\delta$ - at carbon and $\delta$ + at chlorine
D) ionic
E) None of these

Question 59

The C-Cl bond is best described as___________.

A) Nonpolar covalent
B) Polar covalent
C) Ionic
D) Coordinate covalent
E) None of these

Question 60

Which of the following is the correct depiction of induction for a C-F bond?

A) I
B) II
C) III
D) IV
E) None of these

Question 61

Which element has the electron configuration 1s² 2s² 2p⁶ 3s² 3p⁵?

A) oxygen
B) fluorine
C) sulfur
D) chlorine
E) bromine

Question 62

For NaSCH₃, identify each bond as polar covalent, nonpolar covalent or ionic.

Question 63

What is the letter designation for the following atomic orbital?

A) s
B) p
C) d
D) f
E) g

Question 64

In quantum mechanics a node (nodal surface or plane) is:

A) location where $\Psi$ is negative
B) location where $\Psi$ is positive
C) location where $\Psi$ ² is positive
D) location where $\Psi$ ² is negative
E) location where $\Psi$ is zero

Question 65

Orbitals with the same energy are called___________.

A) Quantum orbitals
B) Atomic orbitals
C) Antibonding orbitals
D) Bonding orbitals
E) Degenerate orbitals

Question 66

Which of the following principle states that "Each orbital can accommodate a maximum of two electrons with opposite spin"?

A) Aufbau principle
B) Pauli exclusion principle
C) Hund's Rule
D) Heizenberg Uncertainty principle
E) Le Chatelier principle

Question 67

Which of the following represents ground state electron configuration for phosphorous?

A) 1s² 2s² 2p⁶ 3s¹ 3p⁴
B) 1s² 2s² 2p⁶ 3s² 3p⁴
C) 1s² 2s² 2p⁶ 3s² 3p³
D) 1s² 2s² 2p⁶ 3s² 3p²
E) 1s² 2s² 2p⁶ 3s² 3p⁵

Question 68

For the following compound, identify each bond as polar covalent, nonpolar covalent or ionic and place a $\delta$ + on the most electropositive carbon.

Question 69

Which element has the following electronic configuration?

A) boron
B) carbon
C) silicon
D) nitrogen
E) fluorine

Question 70

Which of the following principle states "When orbitals of equal energy are available, every orbital gets one electron before any gets two electrons"?

A) Aufbau principle
B) Pauli exclusion principle
C) Hund's Rule
D) Heizenberg Uncertainty principle
E) Le Chatelier principle

Question 71

The following ground state electron configuration violates ____.

A) the Aufbau principle
B) the Pauli Exclusion principle
C) Hund's Rule
D) Heisenberg's Uncertainty principle
E) None of these

Question 72

Which element has the electron configuration 1s² 2s² 2p⁶ 3s² 3p³?

A) Cl
B) S
C) P
D) Al
E) N

Question 73

The following ground state electron configuration violates ___.

A) the Aufbau principle
B) the Pauli Exclusion principle
C) Hund's Rule
D) Heisenberg's Uncertainty principle
E) None of these

Question 74

The atomic number for nitrogen is 7. Which of the following represents ground state electron configuration for nitrogen?

A) 1s² 2s¹ 2p⁴
B) 1s² 2p⁵
C) 2s² 2p⁵
D) 1s² 2s² 2p³
E) 1s² 2s² 3s³

Question 75

What is the letter designation for the following atomic orbital?

A) s
B) p
C) d
D) f
E) g

Question 76

What is the electronic configuration for the nitride ion?

A) 1s² 2s² 2p⁰
B) 1s² 2s² 2p²
C) 1s² 2s²2p³
D) 1s² 2s²2p⁴
E) 1s² 2s² 2p⁶

Question 77

The following ground state electron configuration violates ____.

A) the Aufbau principle
B) the Pauli Exclusion principle
C) Hund's Rule
D) Heisenberg's Uncertainty principle
E) None of these

Question 78

What is the electronic configuration for the oxide ion?

A) 1s² 2s² 2p⁶
B) 1s² 2s² 2p²
C) 1s² 2s²2p⁴
D) 1s² 2s⁰2p⁶
E) 1s² 2s² 2p⁶3s²2p²

Question 79

What is the electronic configuration for the magnesium ion?

A) 1s² 2s² 2p⁶3s²
B) 1s² 2s² 2p⁶
C) 1s² 2s²2p⁴
D) 1s² 2s²2p⁶3s¹
E) 1s² 2s² 2p⁶3s²2p²

Question 80

Which element has the following electronic configuration?

A) boron
B) carbon
C) silicon
D) nitrogen
E) fluorine