Test 6

Question 1

what are good examples of atoms with stable electron configurations

Answer 1

noble gases

Question 2

bonding usually __ energy as the atom’s electron configurations attain lower energy states

Answer 2

releases

Question 3

why do atoms with more than 4 valence electrons tend to gain electrons?

Answer 3

they have relatively high electron affinities

Question 4

__ is the tendency of an object to form 2 localized regions of opposite character

Answer 4

polarity

Question 5

can a completely ionic bond result from electron transfer? why? why not?

Answer 5

no, that would imply that the donor atom had no affinity for the donated electrons

Question 6

what is a bonding pair of electrons and where are they found?

Answer 6

the two shared electrons that make up a pair. they are in between the nuclei

Question 7

what is electrostatic force

Answer 7

the force exerted between electrical charges

Question 8

name the natural diatomic elements

Answer 8

Hydrogen, Nitrogen, Oxygen, Fluorine, Chlorine, Bromine, Iodine

Question 9

when using Lewis structures, a __ is substituted for the bonding pair to simplify the diagram

Answer 9

dash

Question 10

in a Lewis structure a dash represents how many electrons?

Answer 10

2

Question 11

The element with the most __ electrons will likely be the central atom

Answer 11

bonding sites/unpaired electrons

Question 12

most polyatomic ions are __, formed by acquiring additional electrons to make up their octet

Answer 12

anions

Question 13

how many atoms can hydrogen have

Answer 13

2

Question 14

what is the hardest natural substance known?

Answer 14

diamond

Question 15

the melting points of ionic compounds are at least__, illustrating just how __ their bonds are. describe ionic compounds

Answer 15

800*C
strong
dense, brittle, and hard solids

Question 16

An __ is a mixture of a metal’s atoms with another element and has metallic properties

Answer 16

alloy

Question 17

what kind of energy moves quickly through metallic objects

Answer 17

thermal

Question 18

the shape of a metal object can be changed by hammering or stretching __ significantly affecting its __

Answer 18

without

strength

Question 19

covalent bonds

Answer 19

Two atoms held together by their mutual attraction for the same pair of electrons. It usu- ally involves two nonmetals

Question 20

ionic bonds

Answer 20

The attraction and electron transfer between two oppositely charged ions in a solid. It usually involves a metal and a nonmetal.

Question 21

metallic bonds

Answer 21

A communal sharing of electrons between metal atoms.

Question 22

A force of attraction produced by transferring or sharing electrons that holds atoms together in compounds.

Answer 22

chemical bonds

Question 23

states that an atom tends to gain, lose, or share electrons until its outer level s and p orbitals are filled with eight electrons. This activity gives an element the electron configuration and stability of a noble gas.

Answer 23

octet rule

Question 24

in covalent bonding…

Answer 24

electrons are shared

Question 25

CNN

Answer 25

covalent nonmetal nonmetal

Question 26

IMN

Answer 26

ionic metal nonmetal

Question 27

MMM

Answer 27

metallic metal metal

Question 28

guidelines for creating Lewis structures

Answer 28

1. Lewis structures illustrate only compounds consisting of covalent bonds. 2. Electron sharing occurs when one nonmetal atom bonds with another (e.g., hydrogen and fluorine) or when two identical nonmetal atoms bond (e.g., fluorine and fluorine). 3. Each nonmetal generally forms covalent bonds to achieve eight electrons in its valence shell, including bonding and nonbonding electrons. Hydrogen is a major exception since its valence shell holds only two electrons. 4. Electrons are normally shared in pairs since two electrons of opposite spin occupy empty orbitals. 5. Polyatomic molecules, which contain three or more atoms, have one or more central atoms bonded to surrounding atoms. Since hydrogen can share only one pair of electrons, it can never be the central atom in a polyatomic molecule. Atoms with valence structures similar to Group 14 atoms (the carbon family) are more likely to be the central atom in a polyatomic molecule. 6. The number of valence electrons for nonmetals (except hydrogen) can be predicted by the formula valence e– = group number – 10. The number of covalent bonds in which nonmetals can participate is predicted by the formula covalent bonds = 8 – valence e–

Question 29

A group of atoms that maintains a constant electrical charge while existing as a unit in a wide variety of chemical reactions

Answer 29

polyatomic ion

Question 30

An extensive three-dimensional structure that represents the regular pattern of atoms or ions

Answer 30

crystal lattice

Question 31

A theory that offers an explanation of how metals bond: the valence electrons of atoms are said to be freely shared among all atoms

Answer 31

electron sea theory--associated with metallic bonds

Question 32

An electron that can move between several different bonds

Answer 32

delocalized electron

Question 33

why do electrons rearrange during bonding?

Answer 33

to maximize stability