Chapter 6 Covalent Bonding

Question 1

What is the name of N2O3?

Answer 1

Dinitrogen trioxide

Question 2

What is the chemical formula for tetrasulfur pentoxide?

Answer 2

S4O5

Question 3

What is the name of C3Cl8

Answer 3

Tricarbon octachloride

Question 4

What is the chemical formula for Nitrogen triiodide?

Answer 4

NI3

Question 5

What is the name of Br6F10 ?

Answer 5

Hexabromine decafluoride

Question 6

What is the chemical formula for Tetraphosphorous Pentachloride ?

Answer 6

P4Cl5

Question 7

What is the name of CO

Answer 7

carbon monoxide

Question 8

What is the chemical formula for Fluorine trisulfide ?

Answer 8

FS3

Question 9

What is the name of S2Br6?

Answer 9

Disulfur hexabromide

Question 10

What is the chemical formula for phosphorus triiodide?

Answer 10

PI3

Question 11

What is the chemical formula for chlorine pentoxide?

Answer 11

ClO5

Question 12

What is the name of P4S5?

Answer 12

Tetraphosphorus pentasulfide

Question 13

What is the name of SeF3?

Answer 13

selenium trifluoride

Question 14

What is the prefix for 1?

Answer 14

mono

Question 15

What is the prefix for 8?

Answer 15

octa

Question 16

What is the prefix for 10?

Answer 16

deca

Question 17

What is the prefix for 4?

Answer 17

tetra

Question 18

covalent compounds contain:

Answer 18

2 nonmetals

Question 19

What is the correct name for C4H6?

Answer 19

tetracarbon hexahydride

Question 20

NH3 has how many lone pairs?

Answer 20

1

Question 21

What is a covalent bond?

Answer 21

A bond formed when two atoms share a pair of electrons

Question 22

In chemical compounds, covalent bonds form when

Answer 22

pairs of electrons are shared between two non-metal atoms.

Question 23

The melting point of sugar is__________________ the melting point of table salt.

Answer 23

less than

Question 24

What are properties of a covalently-bonded compound?

Answer 24

Low melting point, Generally insoluble/immiscible in water, Generally soft and flexible

Question 25

How does the covalent bond form between two atoms?

Answer 25

When the two atoms share electrons

Question 26

Why is the H2 molecule more stable than two separate hydrogen atoms?

Answer 26

Hydrogen only needs two electrons to become stable so when separate hydrogen atoms share their single electrons, it becomes stable

Question 27

Explain why the stability described in item 2 does or does not hold true for most covalent bonds?

Answer 27

The H2 molecule is stable but not true for other bonds because each e- has to have 8 valence electrons except H

Question 28

How does a covalent bond differ from an ionic bond

Answer 28

Covalent bonds share electrons, ionic bonds transfer electrons from one another

Question 29

What is a molecular orbital?

Answer 29

a regions of high probability that is occupied by in individual electron as it travels around two or more associated nuclei

Question 30

Describe the potential energy change that occurs when two hydrogen atoms approach each other and form a covalent bond

Answer 30

The potential energy of two separate hydrogen atoms (right) decreases as they approach each other, and the single electrons on each atom are shared to form a covalent bond.

Question 31

In terms of energy, why is the H-H bond stable?

Answer 31

It is stable because of the shared electrons. Hydrogen only needs two electrons to become stable

Question 32

What is bond length?

Answer 32

The average distance between two bonded atoms at their minimum potential energy

Question 33

What is bond energy?

Answer 33

the energy required to break the chemical bond between two atoms and separate them

Question 34

The tendency of an atom to attract bonding electrons to itself when it bonds with another atom is called ______________

Answer 34

electronegativity

Question 35

_____________is an attraction between two atoms in which electrons are shared equally between atoms.

Answer 35

nonpolar covalent

Question 36

____________is an attraction between two atoms in which bonding electrons are localized on the more electronegative atom.

Answer 36

polar covalent

Question 37

__________ is a molecule in which one end has a partial positive charge and the opposite end has a partial negative charge.

Answer 37

dipole

Question 38

In general, if the difference in electronegativity between two atoms is between 0 and 0.4, the bond is __________.

Answer 38

nonpolar covalent

Question 39

If the electronegativity difference between two atoms is between 0.5 and 1.7, the bond formed is __________.

Answer 39

polar covalent

Question 40

If the electronegativity difference between two atoms is greater than 2.1 the bond formed is __________.

Answer 40

ionic

Question 41

A possible Lewis structure of a molecule for which more than one Lewis structure can be written is called a __________ structure

Answer 41

resonance

Question 42

A structure in which atomic symbols represent nuclei and inner-shell electrons and in which dots are used to represent valence electrons is called a ________ structure.

Answer 42

Lewis

Question 43

explain the difference between single double and triple bonds

Answer 43

A single bond is formed when two atoms share one pair of electrons, whereas a double bond is formed when two atoms share two pairs (four electrons). Three pairs of electrons (six atoms) are shared to form triple bonds.

Question 44

What does the VSEPR theory predict?

Answer 44

The arrangement of electron pairs around each central atom and the correct arrangement of atoms in a molecule.

Question 45

How does one unbonded pair of electrons affect the shape of a molecule?

Answer 45

The electrons in the unbonded pair repel bonding electrons as far away from it as possible.

Question 46

How do multiple unbonded pairs of electrons affect the shape of a molecule?

Answer 46

They can repel each other as well as bonding electrons, forming a bent molecule.

Question 47

What evidence is there to support the idea that opposite polar ends of molecules attract each other?

Answer 47

The energy required to separate polar molecules is greater than that required to separate non polar molecules.

Question 48

How do polarity and shape of molecules relate to the properties of a substance?

Answer 48

They can affect how a molecule fits into another structure and how it tastes. It can also affect how easy the molecule is to separate and its attraction to positively or negatively charged objects.

Question 49

Why is bond length an average rather than a fixed number?

Answer 49

Because bonded atoms can experience vibration causing the bond to stretch and bend.

Question 50

Electron affinity is:

Answer 50

energy change when an electron is acquired by a neutral atom

Question 51

Covalent bonds have a ______ boiling point

Answer 51

low

Question 52

What does the Lewis structure help us see?

Answer 52

The arrangement of electrons in a a molecule

Question 53

As the number of bonds increases in a molecule, the bond length:

Answer 53

decreases

Question 54

Trigonal planar angle:

Answer 54

120

Question 55

Bent angle with one lone pair:

Answer 55

116

Question 56

Tetrahedral angle:

Answer 56

109.5

Question 57

Trigonal pyramidal angle:

Answer 57

107

Question 58

Bent angle with two lone pairs:

Answer 58

105