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Junior 2015-2016 > Chemistry Chapter 6 > Flashcards

Chemistry Chapter 6 Flashcards

1
Q

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

A

chemical bond

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2
Q

what are the types of chemical bonds

A

ionic and covalent

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3
Q

what does an ionic bond do

A

give and take electrons

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4
Q

what does an ionic bond do

A

share electrons

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5
Q

formed by the transfer of one or more electrons which result in the formation of positive and negative ions which are then attracted to each other

A

ionic bond

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6
Q

results from the simultaneous attraction of 2 nuclei for the same electrons resulting in the sharing of the electrons

A

covalent bonds

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7
Q

what is a polar bond?

A

unequal sharing of electron

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8
Q

what is nonpolar bond?

A

equal sharing of electrons

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9
Q

how do you predict bond type

A

use electronegativity difference of the atoms

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10
Q

has the electronegativity difference >1.7

A

ionic

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11
Q

has the electronegativity difference between 0.3 and 1.7

A

polar

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12
Q

has the electronegativity difference

A

nonpolar

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13
Q

ionic of molecular?

all solids

A

ionic

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14
Q

ionic of molecular?

high melting point

A

ionic

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15
Q

ionic of molecular?

do not conduct unless molten or in solution

A

ionic

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16
Q

ionic of molecular?

hard, brittle

A

ionic

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17
Q

ionic of molecular?

may exist as gas, liquid or solids

A

molecular

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18
Q

ionic of molecular?

low melting point

A

molecular

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19
Q

ionic of molecular?

poor heat conductors

A

molecular

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20
Q

ionic of molecular?

good electrical insulators

A

molecular

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21
Q

ionic of molecular?

soft, waxy

A

molecular

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22
Q

composed of positive and negative ions combined so that the net charge of the compound is zero

A

ionic compound

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23
Q

simplest ration of ions in an ionic compound

A

formula unit

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24
Q

ions combining in an orderly arrangement

A

crystal lattice

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25
Q

what does crystal lattice do?

A

reduce energy

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26
Q

group of covalently bonded atoms that carries a change

A

polyatomic ions

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27
Q

phosphate

A

phosphate: PO4^-2

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28
Q

nitrate

A

nitrate: NO3^-1

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29
Q

hydroxide

A

hydroxide: OH^-1

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30
Q

sulfate

A

sulfate: SO4^-2

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31
Q

ammonium

A

ammonium: NH4^+1

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32
Q

consists of an agreement of positive ions that are located at the crystal lattice sites and are immersed in a “sea” of mobile electrons

A

metallic bond

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33
Q

what does the mobility of electrons result in?

what are these things?

A

metallic properties

  • good conductor of electricity and heat
  • malleability
  • ductility
  • luster
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34
Q

what does the strength of metal vary with?

A

the nuclear charge and the number of valence electrons

35
Q

neutral group of atoms held together by covalent bonds

A

molecule

36
Q

shows the types and number of atoms combined in a single molecule of a molecular compound

A

molecular formula

37
Q

what is the formation of a covalent bond?

A

there is a release of energy when bonds are formed, resulting in a lower energy system and more stable system

38
Q
  • the ____ energy given _____ the more stable the compound the _____ the bond
  • the _____ energy given off the _____stable the compound the _____ bond
A

more, more, stronger

less, less, weaker

39
Q

energy required to break a chemical bond and form neutral isolated atoms

A

bond energy

40
Q

compounds form that each atom, by gaining, losing or sharing electrons, has an octet of electrons in its outer energy level

A

the octet rule

41
Q

uses dots to show the valence electrons for an element

A

dot notation

42
Q

uses symbol of each element in the compound and dot pairs or dashes between atoms to represent shared electrons and dots next to a symbol to represent unshared electrons

A

lewis structures

43
Q

indicates the kind, #, arrangement, and bonds but not the unshared pairs of the atoms in a molecule

A

structural formula

44
Q

sharing only one pair of electrons between atoms

A

compounds with single covalent bonds

45
Q

sharing 2 pairs of electrons between two atoms

A

double bonds

46
Q

sharing 3 pairs of electrons between 3 atoms

A

triple bonds

47
Q

(17)

A

linear

48
Q

(16)

A

angular

49
Q

(15)

A

pyramidical

50
Q

(14)

A

tetrahedral

51
Q

an uneven distribution of electrical charge in a molecule

-causes a molecule to be polar and result in the strongest inter molecular forces-higher boiling point

A

dipole

52
Q

a special dipole
dipole force
results because _____ and another highly electronegative atom pulls _____ electron very close to it, leaving an almost bare proton
-accounts for the high boiling point of water, low vapor pressure and low density of ice

A

hydrogen bond

53
Q

in _____ molecules, weak attractive forces exist between molecules

  • results from momentary dipoles as electrons move about the atom
  • makes it possible for small ____ molecules to exist as liquids or solid under conditions of lower temperature and high pressure
A

nonpolar

54
Q

boiling point and bond tyype

A

nonpolar covalent

55
Q

an atom that gains one or more electrons will have a _____ charge

A

negative

56
Q

an atom that loses one or more electrons will have a ____ charge

A

positive

57
Q

an atom that gains or loses one or more electrons is called an ____

A

ion

58
Q

a positive ion is called a ____ and a negative ion is called an _____

A

cation

anion

59
Q

atoms will transfer one or more ____ to another to form the bond

A

electrons

60
Q

each atom is left with a ____ outer shell

A

complete

61
Q

an ionic bond forms between a ____ ion with a positive charge and a ____ ion with a negative charge

A

metal

nonmetal

62
Q

atoms ___ one or more electrons with each other to form the bond

A

share

63
Q

each atom is left with a ____ outer shell

A

complete

64
Q

a covalent bond forms between two _____

A

nonmetals

65
Q

the charge on an ion is

A

either positive or negative

66
Q

what is a polyatomic ion

A

has many ions with a charge

67
Q

the crystal structure of an ionic compound depends on the ___ and ____ of the cations and anion

A

sizes and ratio

68
Q

the melting points of ionic compounds are higher than the melting points of molecular compounds because

A

attractive forces between ions are greater than the attractive forces between molecules

69
Q

a covalent bond is formed when two atoms

A

share one or more electrons with each other

two electrons have to be made

70
Q

how many double bonds are in the lewis structure for hydrogen fluoride HF

A

none

71
Q

two atoms will likely form a polar covalent bond if the electronegativity difference is

A

between 0.3 and 1.7

72
Q

in a double covalent bond

A

two atoms share two pairs of electrons

73
Q

the boiling point of water, H2O is higher than the boiling point of sulfide H2S because water molecules are…

A

more polar and form hydrogen bonds

74
Q

which type of bonding is characterized by overlapping orbital that allow outer electrons of atoms to move about freely throughout the entire lattice

A

metallic

75
Q

according to VESPR what is the shape of a molecule of CS2

A

linear

76
Q

according to VESPR theory, what is the shape of a molecule of NBr3

A

pyramidal

77
Q

an ionic bond results from electrical attraction between

A

cations and anions

78
Q

a nonpolar covalent bond is unlikely when two atoms of different elements join because the atoms are likely to differ in

A

electronegativity

79
Q

if two covalently bonded atoms move closer than a distance of the bond length, the potential energy of the atoms

A

increase

80
Q

for multiple covalent bonds to form in molecules, the molecules mus contain carbon, nitrogen, or

A

oxygen

81
Q

the principle that states that atoms tend to form compounds in which each atom has eight electrons in its highest occupied energy level is called the

A

octet rule

82
Q

lattice energy is an indication of the

A

strength of an ionic bond

83
Q

explain the intermolecular force that contributes to the high boiling point of water

A

results because hydrogen and another highly electronegative atom pulls hydrogen electron very close to it, leaving an almost bare proton

84
Q

compare and contast ionic bonding and covalent bonding

A

ionic bonds are formed from one or more electrons and covalent bonds are bonded by the same electron. Ionic bonds from simultaneous attraction ionic of positive and negative ions, and covalent attraction of 2 nuclei

Junior 2015-2016 (15 decks)

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