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

What is the correct Lewis dot structure for S?

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

Answer 2

III

Question 3

What is the correct Lewis structure for CH₃CO₂H?

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

Answer 3

IV

Question 4

What is the difference between inorganic and organic compounds?

A) organic compounds do not contain carbon
B) organic compounds contain carbon
C) organic compounds are without pesticides
D) inorganic compounds contain carbon
E) inorganic compounds are composed exclusively of transition metal elements

Question 5

What is the relationship between the following compounds?

A) resonance isomers
B) constitutional isomers
C) empirical isomers
D) There is no relationship

Question 6

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

A) CO₂
B) SCl₂
C) NF₃
D) CS₂
E) SO₃

Question 7

Carbon is considered to be _______.

A) tetravalent
B) divalent
C) trivalent
D) monovalent
E) pentavalent

Question 8

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

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

Question 9

What is the relationship between the following compounds?

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

Question 10

What is the correct Lewis structure for COCl₂?

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

Question 11

Constitutional isomers do not differ in ____________.

A) physical properties
B) atomic connectivity
C) molecular formula
D) name
E) constitution

Question 12

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

A) I and II
B) III and IV
C) I, II and IV
D) II, III and IV
E) I, II, and III

Question 13

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

A) repulsion between two positively charged nuclei
B) force of attraction between positively charged nuclei and negatively charged electrons
C) repulsion between two negatively charged nuclei
D) repulsion between positively charged nuclei and negatively charged electrons

Question 14

Draw three constitutional isomers that have molecular formula C₄H₈O.

Question 15

Chemical reactions occur as a result of __________

A) the attraction between opposite charges.
B) the nucleus-nucleus interactions.
C) the motion of electrons.
D) like atoms interacting.
E) combining two chemicals.

Question 16

Draw three constitutional isomers that have molecular formula C₄H₈BrCl

Question 17

From the following, identify the item which does not contain organic compounds.

A) medicine
B) socks
C) a plant
D) a coin
E) a plastic cup

Question 18

What is the correct Lewis dot structure for C?

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

Question 19

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

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

Question 20

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

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

Question 21

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 22

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

Question 23

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

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

Question 24

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

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

Question 25

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 26

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 27

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

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

Question 28

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 29

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 30

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 31

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

Question 32

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

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

Question 33

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

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

Question 34

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

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

Question 35

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 36

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

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

Question 37

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 38

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

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

Question 39

In an 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 40

Draw the Lewis structure for ^-CH₂CN including formal charges?

Question 41

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 42

For the following compound identify the polar covalent bonds and indicate the partial charges by using $\delta$ + and $\delta$ -.

Question 43

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

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

Question 44

For the following compound identify the polar covalent bonds and indicate the partial charges by using $\delta$ + and $\delta$ -.

Question 45

Which of the following is the most electronegative element?

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

Question 46

Which of the following is the least electronegative element?

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

Question 47

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

Question 48

The Cl-Cl bond is best described as___________.

A) nonpolar covalent
B) polar covalent
C) ionic
D) coordinate covalent
E) None of these.

Question 49

The C-Cl bond 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 compounds have both polar covalent and ionic bonds?

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

Question 51

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 52

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) from upper right to lower left

Question 53

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

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

Question 54

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 55

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 56

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 57

Which of the following is the most electronegative element?

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

Question 58

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 59

Which of the following is the least electronegative element?

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

Question 60

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 61

The atomic number for nitrogen is 7. Which of the following represents the 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 62

Which of the following represents the 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 63

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

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

Question 64

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

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

Question 65

Ar, K⁺, and Cl^- have equal numbers of electrons, and are considered isoelectronic. Provide the ground state electron configuration for them.

Question 66

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 67

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's principle

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

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 70

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's principle

Question 71

What is the letter designation for the following atomic orbital?

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

Question 72

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 73

Orbitals with the same energy are called ___________.

A) quantum orbitals
B) atomic orbitals
C) antibonding orbitals
D) bonding orbitals
E) degenerate orbitals

Question 74

Which element has the following electronic configuration?

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

Question 75

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 76

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

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

Question 77

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 78

Which element has the following electronic configuration?

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

Question 79

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 80

What is the letter designation for the following atomic orbital?

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