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Week 5 - Chemistry

front 1

In a covalent bond

A) two atoms exchange electrons and the ions are attracted to one another.

B) two ions come together and form a crystal lattice.

C) two atoms share valence electrons and those shared electrons form the chemical bond.

D) two elements react and form a new compound.

back 1

C) two atoms share valence electrons and those shared electrons form the chemical bond.

front 2

Which of the following is an example of a covalent bond?

A) K - Cl

B) Al - Cl

C) H - Cl

D) Al - Al

back 2

C) H - Cl

front 3

What is the correct IUPAC name for BrCl₃?

back 3

bromine trichloride

front 4

What is the correct IUPAC name for CBr₄?

back 4

carbon tetrabromide

front 5

What is the correct IUPAC name for CBr₄?

back 5

carbon tetrabromide

front 6

What is the correct IUPAC name for NI₃?

back 6

nitrogen triiodide

front 7

What is the correct IUPAC name for N₂O₄?

back 7

dinitrogen tetroxide

front 8

What is the correct IUPAC name for P₄S₃?

back 8

tetraphosphorus trisulfide

front 9

What is the correct IUPAC name for SeO₂?

back 9

selenium dioxide

front 10

What is the correct IUPAC name for S₂Cl₈?

back 10

disulfur octachloride

front 11

What is the correct IUPAC name for TeBr₆?

back 11

tellurium hexabromide

front 12

What is the correct IUPAC name for Se₂I₈?

back 12

diselenium octaiodide

front 13

What is the correct IUPAC name for SO₃?

back 13

sulfur trioxide

front 14

What is the correct IUPAC name for TeF₄?

back 14

tellurium tetrafluoride

front 15

What is the correct IUPAC name for AsBr₃?

back 15

arsenic tribromide

front 16

What is the correct IUPAC name for As₂S₅?

back 16

diarsenic pentasulfide

front 17

What is the correct IUPAC name for SbCl₃?

back 17

antimony trichloride

front 18

Write the chemical formula for arsenic pentafluoride

back 18

AsF₅

front 19

Write the chemical formula for bromine pentachloride

back 19

BrCl₅

front 20

Write the chemical formula for carbon tetrafluoride

back 20

CF₄

front 21

Write the chemical formula for dichlorine heptoxide

back 21

Cl₂O₇

front 22

Write the chemical formula for dinitrogen tetroxide

back 22

N₂O₄

front 23

Write the chemical formula for diphosphorus pentabromide

back 23

P₂Br₅

front 24

Write the chemical formula for nitrogen trichloride

back 24

NCl₃

front 25

Write the chemical formula for selenium hexafluoride

back 25

SeF₆

front 26

Write the chemical formula for sulfur tetraiodide

back 26

SI₄

front 27

Write the chemical formula for tellurium hexaiodide

back 27

TeI₆

front 28

Write the chemical formula for tetraphosphorus hexasulfide

P₄S₆

back 28

P₄S₆

front 29

Which has the correct name-formula combination?

A) Chlorine pentafluoride - ClF

B) Diphosphorus pentoxide - P₂O

C) Carbon tetraiodide - CI₄

D) Sulfur tetrafluoride - SF

back 29

C) Carbon tetraiodide - CI₄

front 30

Which has the incorrect name-formula combination?

A) Sulfur dioxide - SO₂

B) Iodine trifluoride - IF

C) Nitrogen tribromide - NBr₃

D) Silicon tetrafluoride - SiF₄

back 30

B) Iodine trifluoride - IF

front 31

Which of the following is the correct Lewis symbol for a neutral atom of Al?

A) see problem image

B) see problem image

C) see problem image

D) see problem image

back 31

C) see problem image

front 32

Which of the following is the correct Lewis symbol for a neutral atom of F?

A) see problem image

B) see problem image

C) see problem image

D) see problem image

back 32

B) see problem image

front 33

Which of the following is the correct Lewis symbol for a neutral atom of O?

A) see problem image

B) see problem image

C) see problem image

D) see problem image

back 33

D) see problem image

front 34

Which of the following is not a valid Lewis symbol?

A) see problem image

B) see problem image

C) see problem image

D) see problem image

back 34

D) see problem image

front 35

Draw the Lewis structure of ammonia (NH₃).

back 35

front 36

Draw the Lewis structure of carbon dioxide (CO₂).

back 36

front 37

Draw the Lewis structure of Cl₂.

back 37

front 38

Draw the Lewis structure of formaldehyde (H₂CO).

back 38

front 39

Draw the Lewis structure of H₂.

back 39

front 40

Draw the Lewis structure of N₂.

back 40

front 41

Draw the Lewis structure of O₂.

back 41

front 42

Draw the Lewis structure of water (H₂O).

back 42

front 43

A skeletal structure for SO₂Cl₂ is shown below. Starting from this structure, complete the Lewis structure that follows the octet rule on all atoms.

back 43

front 44

Determine the number of valence electrons in HCN and then draw the corresponding Lewis structure.

A) 13

B) 12

C) 10

D) 9

E) 7

back 44

C) 10

front 45

Determine the number of valence electrons in POCl₃ and then draw the corresponding Lewis structure (by following the octet rule on all atoms).

A) 30

B) 32

C) 28

D) 31

E) 35

back 45

B) 32

front 46

The Lewis structure for NI₃ shown below is incorrect. Starting from this structure, complete the correct structure.

back 46

front 47

The Lewis structure for SiS₂ shown below is incorrect. Starting from this structure, complete the correct structure.

back 47

front 48

Determine the number of valence electrons in ethene (C₂H₄) and then draw the corresponding Lewis structure.

A) 11

B) 13

C) 12

D) 15

E) 14

back 48

C) 12

front 49

The Lewis structure for ethyne (C₂H₂) shown below is incorrect. Starting from this structure, complete the correct structure.

back 49

front 50

Determine the number of valence electrons in nitrous acid (HNO₂, sometimes written as HONO) and then draw the corresponding Lewis structure.

A) 22

B) 18

C) 19

D) 15

E) 17

back 50

B) 18

front 51

A single bond, compared to a double bond,

A) is longer.

B) is stronger.

C) has a higher bond dissociation energy.

D) is not capable of rotation.

back 51

A) is longer.

front 52

Which of the following has the shortest bond length?

A) a single bond

B) a double bond

C) a triple bond

back 52

C) a triple bond

front 53

Which of the following has the shortest bond length?

A) a single bond

B) a double bond

C) a triple bond

back 53

C) a triple bond

front 54

Which one of the following statements best describes electronegativity in atoms?

A) Electronegativity is what happens when an atom gains an electron to become an anion.

B) Electronegativity is the attraction an element's nucleus has for the electrons in a chemical bond.

C) Electronegativity is the energy lost when an atom gains an electron.

D) Electronegativity is the energy absorbed when an atom loses an electron.

back 54

B) Electronegativity is the attraction an element's nucleus has for the electrons in a chemical bond.

front 55

Which one of the following is the least electronegative atom?

A) Na

B) Cl

C) P

D) Al

back 55

A) Na

front 56

Which group in the periodic table tends to have high electronegativity values?

A) the alkali metals

B) the noble gases

C) the halogens

D) the transition metals

back 56

C) the halogens

front 57

Which of the following bonds is a nonpolar covalent bond?

A) H - F

B) N - F

C) F - Cl

D) F - F

back 57

D) F - F

front 58

Which of the following bonds is a polar covalent bond?

A) Li - Cl

B) Cl - Cl

C) H - Cl

D) Li - Li

back 58

C) H - Cl

front 59

Based on their positions in the periodic table, which of the following bonds is the most polar?

A) O - F

B) C - F

C) B - F

D) F - F

back 59

C) B - F

front 60

In a polar covalent bond,

A) both atoms in the bond have the same level of electronegativity.

B) one atom in the bond must have higher electronegativity than the other atom.

C) one atom must be a H atom.

D) both atoms in the bond must be metals.

back 60

B) one atom in the bond must have higher electronegativity than the other atom.

front 61

Which one of the following statements is FALSE?

A) Ionic bonding results from the transfer of electrons from one atom to another

B) Dipole moments result from the unequal distribution of electrons in a molecule

C) The electrons in a polar bond are found nearer to the more electronegative element

D) A molecule with very polar bonds can be nonpolar

E) Linear molecules cannot have a net dipole moment

back 61

E) Linear molecules cannot have a net dipole moment

front 62

What is the correct molecular geometry of NH₃ according to Valence Shell Electron Pair Repulsion Theory?

A) trigonal planar

B) trigonal pyramidal (pyramidal)

C) bent

D) tetrahedral

back 62

B) trigonal pyramidal (pyramidal)

front 63

Draw the Lewis structure of chloroform (CHCl₃) and then determine the ideal bonding angle(s) of the central atom.

A) 180º

B) 90º and 120º

C) 109.5º

D) 120º

E) 135º

back 63

C) 109.5º

front 64

Draw the Lewis structure of CHOCl and then determine the ideal bonding angle(s) of the central atom.

A) 120º

B) 45º

C) 135º

D) 90º

E) 60º

back 64

A) 120º

front 65

Draw the Lewis structure of ClF₃ (with minimized formal charges) and then determine its electron domain and molecular geometries.

A) trigonal bipyramidal / pentagonal

B) trigonal bipyramidal / t-shaped

C) trigonal / pyramidal

D) trigonal / square planar

E) pyramidal / pentagonal

back 65

B) trigonal bipyramidal / t-shaped

front 66

Draw the Lewis structure of ethyne (C₂H₂) and then choose the appropriate pair of molecular geometries of the two central atoms. Your answer choice is independent of the orientation of your drawn structure.

A) linear / linear

B) trigonal / pyramidal

C) pyramidal / trigonal

D) trigonal pyramidal / trigonal pyramidal

E) planar / linear

back 66

A) linear / linear

front 67

Draw the Lewis structure of H₂CS and then determine its electron domain and molecular geometries.

A) planar / tetrahedral

B) trigonal planar / linear

C) trigonal / trigonal planar

D) trigonal planar / trigonal planar

E) planar / planar

back 67

D) trigonal planar / trigonal planar

front 68

Draw the Lewis structure of methanol (CH₃OH) and then choose the appropriate pair of molecular geometries of the two central atoms. Your answer choice is independent of the orientation of your drawn structure.

A) bent (109.5º) / bent (120º)

B) tetrahedral / bent (109.5º)

C) trigonal pyramidal / planar

D) planar / trigonal

E) bent (120º) / planar

back 68

B) tetrahedral / bent (109.5º)

front 69

Draw the Lewis structure of ozone (O₃) and then determine its electron domain and molecular geometries.

A) planar / trigonal planar

B) trigonal planar / bent (120º)

C) trigonal / trigonal planar

D) planar / trigonal

E) pyramidal / pyramidal

back 69

B) trigonal planar / bent (120º)

front 70

Draw the Lewis structure of PH₃ and then determine its electron domain and molecular geometries.

A) tetrahedral / bent (109.5º)

B) tetrahedral / trigonal pyramidal

C) trigonal / tetrahedral

D) planar / trigonal pyramidal

E) trigonal planar / trigonal planar

back 70

B) tetrahedral / trigonal pyramidal

front 71

Draw the Lewis structure of silicon dioxide (SiO₂) and then determine its electron domain and molecular geometries.

A) planar / trigonal pyramidal

B) trigonal planar / bent (120º)

C) planar / trigonal

D) linear / pyramidal

E) linear / linear

back 71

E) linear / linear

front 72

Draw the Lewis structure of water (H₂O) and then determine its electron domain and molecular geometries.

A) trigonal planar / trigonal

B) trigonal planar / planar

C) tetrahedral / bent (109.5º)

D) tetrahedral / linear

E) tetrahedral / trigonal planar

back 72

C) tetrahedral / bent (109.5º)

front 73

Which of the following bonds is the most polar?

A) P - S

B) C - Cl

C) F - F

D) Rb - Br

E) All bonds have equal polarity.

back 73

D) Rb - Br

front 74

Draw the Lewis structure of carbon dioxide (CO₂) and then determine if the molecule is polar or nonpolar.

A) Nonpolar

B) Polar

back 74

A) Nonpolar

front 75

Draw the Lewis structure of carbon tetrafluoride (CF₄) and then determine if the molecule is polar or nonpolar.

A) Nonpolar

B) Polar+

back 75

A) Nonpolar

front 76

Draw the Lewis structure of formaldehyde (H₂CO) and then determine if the molecule is polar or nonpolar.

A) Nonpolar

B) Polar

back 76

B) Polar

front 77

Draw the Lewis structure of O₂ and then determine if the molecule is polar or nonpolar.

A) Nonpolar

B) Polar

back 77

A) Nonpolar

front 78

Draw the Lewis structure of water (H₂O) and then determine if the molecule is polar or nonpolar.

A) Nonpolar

B) Polar+

back 78

B) Polar

front 79

Draw the Lewis structure of PBr₃ and then determine if the molecule is polar or nonpolar.

A) Nonpolar

B) Polar

back 79

B) Polar

front 80

How would you determine the formula weight of NaCl?

A) Add the mass of sodium (22.99 amu) plus the mass of chlorine together (35.45 amu).

B) Multiply the mass of sodium (22.99 amu) by the mass of chlorine (35.45 amu).

C) Divide the mass of chlorine (35.45 amu) by the mass by sodium (22.99 amu).

D) Subtract the mass of chlorine (35.45 amu) from the mass of sodium (22.99 amu).

back 80

A) Add the mass of sodium (22.99 amu) plus the mass of chlorine together (35.45 amu).

front 81

What are the similarities in how formula weight and molar mass are calculated?

A) Formula weight and molar mass are both calculated by taking the individual atoms' masses in the formula, multiplying them by how many there are in the formula, and then adding the numbers together.

B) Formula weight and molar mass are both calculated by taking the individual atoms' masses in the formula, multiplying them by how many there are in the formula, and then subtracting the numbers from each other.

C) Formula weight and molar mass are both calculated by taking the individual atoms' masses in the formula, dividing them by how many there are in the formula, and then adding the numbers together.

D) Formula weight and molar mass are both calculated by taking the individual atoms mass in the formula, dividing them by how many there are in the formula, and then subtracting the numbers from each other.

back 81

A) Formula weight and molar mass are both calculated by taking the individual atoms' masses in the formula, multiplying them by how many there are in the formula, and then adding the numbers together.

front 82

Determine the formula weight of KBr.

back 82

119.00 amu

front 83

Determine the molar mass of CH₃OCH₃.

back 83

46.08 g/mol

front 84

Determine the molar mass of CH₃OH.

back 84

32.05 g/mol

front 85

Determine the molar mass of C₆H₁₂O₆.

back 85

180.18 g/mol

front 86

Which one of the following has the smallest molar mass?

A) Ca(NO₃)₂

B) Ca₃N₂

C) Ca(C₂H₃O₂)₂

D) CaSO₄

back 86

D) CaSO₄

front 87

The number of covalent bonds carbon forms in organic compounds is ____.

A) 2

B) 3

C) 4

D) 5

E) 6

back 87

C) 4

front 88

Which of the following formulas represents an organic compound?

A) KCl

B) NH₃

C) Cl₂

D) C₃H₈

E) SiH₄

back 88

D) C₃H₈

front 89

A hydrocarbon is referred to as __________ if all the bonds in the molecule are single bonds.

A) aromatic

B) saturated

C) unsaturated

D) planar

E) octahedral

back 89

B) saturated