Chapter 6 Test

Front 1

a mutual electrical attraction between the nuclei and valence electrons of different atoms that binds the atoms toggether

Back 1

chemical bond

Front 2

a chemical bond resulting from the sharing of an electron pair between two atoms

Back 2

covalent bonding

Front 3

the chemical bond resulting fom electrical attraction between large numbers of cations and anions

Back 3

ionic bonding

Front 4

a covalent bond in which the bonding electrons are shared equally by the bonded atoms resulting in the balanced distribution of electrical charge

Back 4

nonpolar covalent bond

Front 5

having an uneven distribution of charge

Back 5

polar

Front 6

a covalent bond in which the baonded atoms have an unequal attraction for the shared electrons

Back 6

polar-covalent bond

Front 7

the energy required to break a chemical bond and from neutral isolated atoms

Back 7

bond energy

Front 8

the distance between two bonded atoms at their minimal potential energy, that is, the average distance between two bonded atoms

Back 8

bond length

Front 9

a formula that indicates the relative numbers of atoms of each kind in a chemical compound by using atomic symbols and numberical subscripts

Back 9

chemical formula

Front 10

a molecule containing only two atoms

Back 10

diatomic molecule

Front 11

a covalent bond produced by the sharing of two pairs of electrons between two atoms

Back 11

double bond

Front 12

an ellectron configuration notation in which only the valence electrons of an atom of a particular elements are shown, indicated by the dots placed around the element's symbol

Back 12

electron-dot notation

Front 13

a formula in which atomic symbols represent nuclei and inner shell electrons dot pairs or dashes between two atomic symbols represents electron pairs in covalent bonds and dots adjacent to only one atomic symbol represent uncharged electrons

Back 13

Lewis structure

Front 14

a pair of electrons that is not involved in bonding and that belongs exclusively to one atom

Back 14

lone pair

Front 15

a chemical compound whose simplest units are molecules

Back 15

molecular compound

Front 16

a formula showing the types and numbers of atoms combined in a single molecule of a molecular compound

Back 16

molecular formula

Front 17

a neutral group of atoms that are held together by covalent bonds

Back 17

molecule

Front 18

a double or triple bond

Back 18

multiple bond

Front 19

chemical compounds tend to form so that each atom, by gaining, losing, or sharing electrons, has an octet of electrons in its hightest occupied energy level

Back 19

octet rule

Front 20

the bonding in molecules or ions that cannot be correctly represented by a single Lewis Structure

Back 20

resonance

Front 21

a covalent bond produced by the sharing of one pair of electrons between two atoms

Back 21

single bond

Front 22

a formula that indicates the number and types of atoms present in a molecule and also shows the bonding arrangement of the atoms; a formulat that indicates the kind, number, arrangement, and bonds but not the unshared electron pair of the atoms in a molecule

Back 22

structural formula

Front 23

a covalent bond produced by the sharing of three pairs of electrons between two atoms

Back 23

triple bond

Front 24

a pair of electrons that is not involved in bonding and that belongs exclusivelt to one atom

Back 24

unshared pair

Front 25

the simplest collection of atoms from which an ionic compound's formula can be established

Back 25

formulat unit

Front 26

a compound composed of positive and negative ions that are combined so that the numbers of positive nad negative charges are equal

Back 26

ionic compound

Front 27

the energy released when one mole of an ionic crystalline compound is formed from gaseous ions

Back 27

lattice energy

Front 28

a charged group of covalencely bonded atoms

Back 28

polyatomic ion

Front 29

the ability of a substance to be drawn puled or extruded trhough a small opening to produce a wire

Back 29

ductibilty

Front 30

the ability of a substance to be hammered into sheets

Back 30

malleability

Front 31

chemical bonding that results from the attraction between metal atoms and the surrounding sea of electroons

Back 31

metallic bonding

Front 32

equal but opposite charges that are separated by a short distance

Back 32

dipole

Front 33

orbitals of equal energy produced by the combinatinos of two or more orbitals on the same atom

Back 33

hybrid orbitals

Front 34

a force of attraction between polar molecules

Back 34

dipole-dipole force

Front 35

the mixing of two or more atomic orbitals of similar energies on the same atom to produce new orbitals of equal energies

Back 35

hybridization

Front 36

the intermolectular force in which a hydrogen atom that is bonded to a hightly electronegative atom is attracted to an unshared pair of electrons of an electronegative atom in a nearby molecule

Back 36

hydrogen bonding

Front 37

the force of attraction between molecules

Back 37

intermolecular force

Front 38

the uneven distribution of molecular charge

Back 38

molecular polarity

Front 39

in a chemical bond the link between atoms results from the attraction between electrons and

Back 39

nuclei

Front 40

a covalent bond consists of

Back 40

a shared electron pair

Front 41

if two covalently bonded atoms are identical the bond is identified as

Back 41

nonpolar covalent

Front 42

a covalent bond in which there is an unequal attraction for the shared electrons is

Back 42

polar

Front 43

atoms with a stron attraction for electrons they share with another atom exhibit

Back 43

high electronegativity

Front 44

bonds with between 5% and 50% ionic character are considered to be

Back 44

polar covalent

Front 45

a nonpolar covalent bond is likely to exist between

Back 45

two identical atoms

Front 46

the greater the electronegativity difference between two bonded atoms the greater the percentage of

Back 46

ionic character

Front 47

the electrons involved in the formation of a chemiucal bond are called

Back 47

valence electrons

Front 48

a chemical bond resulting from electronstatic attraction between positive and negative ions is called an

Back 48

ionic bond

Front 49

if the electrons involved in bonding spend most of the time close to one atom rather than the toher the bond is

Back 49

polar covalent

Front 50

a chemical bond that results from the electrostatic attraction between positive and negative ions is called an

Back 50

ionic bond

Front 51

if electrons involved in bondnig spend most of the time closer to one atom rather thatn the other the bond is

Back 51

polar covalent

Front 52

if a bond's character is more than 50% ionic if the electronegativity difference between the two atoms is greater than

Back 52

1.7

Front 53

a large difference in electronegativity between two atoms in a bond results in

Back 53

ionic bonding

Front 54

what happens when atoms bond with each other

Back 54

they creeate arrangements of matter that are more stable

Front 55

the type of bond that shares electrons

Back 55

covalent

Front 56

elements that lose electrons and form positive ions

Back 56

metals

Front 57

metal-nonmetal bond

Back 57

ionic

Front 58

elements that gain electrons and from negative ions

Back 58

nonmetals

Front 59

electrons in the outermost energy levels

Back 59

valence electrons

Front 60

type of bond that transfers electrons

Back 60

ionic bond

Front 61

this bond forms compounds with low melting points

Back 61

molecular

Front 62

nonmetal nometal bond

Back 62

covalent

Front 63

this bond forms crystalline compounds

Back 63

ionic bond

Front 64

an atom or ion with a full outer energy level has a

Back 64

octet

Front 65

when an atom of one element combines chemically with an atom of another element both atoms usually attain the stable highest energyy level configuratin of a

Back 65

noble gas

Front 66

in a molecule of fluprine the two shared electrons give each fluoroing atom ___ electrson in the outer energy level

Back 66

8

Front 67

in writing a lewis structure each nonmetal atom except hydrogen shuld be surrounded by

Back 67

8 electrons

Front 68

in writing a lewis structure the central atom is the

Back 68

least electronegative atom

Front 69

to draw the electron-dot symbols for each atom in a lewis structure one must know the

Back 69

number of valence lectrons in each atom

Front 70

nature favors chemical bonding because

Back 70

potential energy is minimized when atoms are bonded

Front 71

when atoms are drawn together by attractive forces their potential energy

Back 71

is decreased

Front 72

potential energy is at a minium when

Back 72

the repulsion between the like charges equal the attraction of the opposite charges

Front 73

atoms are drawn to each other because the electron-proton attraction

Back 73

is stronger than the electron-electron and proton-proton repulsions

Front 74

the molecular formula H20 indicates a molecule

Back 74

with two atoms of hydrogen bonded with one atom of oxygen

Front 75

the strength of attraction between charged particles depends on the distance between the atoms involved in the bonds. tf

Back 75

true

Front 76

the bond length is the distance between two bonded atoms at their maximum potential energy

Back 76

false

Front 77

the energy required to form a chemical bond between to neutral atoms is called bond energy

Back 77

false

Front 78

according to the octet rule chemical compounds tend to form so that each atom has an octet of electrons in tis hightes energy level

Back 78

true

Front 79

when the orbitals of the hydrogen atoms in a hydrogen molecule overlap the electron density between the nuclei decreases

Back 79

false

Front 80

in the formula for sodium chloride NaCl stands for one

Back 80

formula unit

Front 81

the chemical formula for an ionic compound represents the

Back 81

simplest ratio of the combined ions that gives neutrality

Front 82

in a crystal of an ionic compound, each catino is surrounded bby a number of

Back 82

anions

Front 83

in a crystal the valence electrons of adjacent ions

Back 83

neutralize each other

Front 84

compared to the neutral atoms involved in its formationthe crystal lattice that results is

Back 84

lower in potential energy

Front 85

which of the following is NOT a proprerty of an ionic compound

Back 85

vaporizes at room temp

Front 86

compared to ionic compounds molecular compounds have

Back 86

lower melting points

Front 87

the forces of attraction between molecules ina molecular compound are

Back 87

weaker than the forces of ionif bonding

Front 88

at room temperature most ionic compounds will be

Back 88

solids

Front 89

molecular compounds are ____ at room temperature

Back 89

completely gaseous

Front 90

which is true of ionic compounds

Back 90

the ions cannot move in the solid structure

Front 91

NaCl is a molecular compound

Back 91

false

Front 92

lattice energy is released when the ions in a crystal lattice are separated from each each otther

Back 92

false

Front 93

ionic compounds are electrical conductors in their molten staes

Back 93

true

Front 94

an ionic compound is compose dof independent netural elements that can be isolated from each other

Back 94

false

Front 95

the atoms in molecular compounds are held together by covalent bonds

Back 95

true

Front 96

calculating lattice energies helps chemists compare bond strentgths in ionic compounds

Back 96

true

Front 97

a polyatomic ion with a shortage of electrons has a positive charge

Back 97

true