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chemistry 1 > Chemical Bonding > Flashcards

Chemical Bonding Flashcards

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1
Q

chemical bond

A

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

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2
Q

purpose of chemical bonds

A

decrease potential energy of atoms

increase stability of atoms

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3
Q

types of chemical bonds

A

ionic bond

covalent bond

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4
Q

difference between types of chemical bonds

A

the way the electrons are redistributed

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5
Q

ionic bond

A

the transfer of electrons to other atoms

results from the electrical attraction between large numbers of cations and anions

bond between atoms with an electronegativity difference of 1.7 or greater

formed between metals and nonmetals

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6
Q

covalent bond

A

the sharing of electrons between two bonded atoms

bond between atoms with an electronegativity difference of 1.7 or less

formed between nonmetals

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7
Q

determining factor of type of chemical bond

A

difference in the bonded atoms’ electronegativities

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8
Q

type of bond between atoms of the same element

A

covalent bond

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9
Q

types of covalent bonds

A

nonpolar covalent bond

polar covalent bond

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10
Q

nonpolar covalent bond

A

covalent bond in which the bonding electrons are shared equally by the bonded atoms

results in a balanced distribution of electrical charge

bond between atoms with an electronegativity difference between 0.0 and 0.3

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11
Q

polar covalent bond

A

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

results in an imbalanced distribution of electrical charge

bond between atoms with an electronegativity difference between 0.3 and 1.7

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12
Q

molecule

A

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

simplest unit of a molecular compound

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13
Q

molecular compound

covalent compound

A

chemical compound formed by two or more bonded atoms through the sharing of electrons

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14
Q

chemical formula

A

indication of the relative numbers of atoms of each kind in a chemical compound by using atomic symbols and numerical subscripts

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15
Q

molecular formula

A

chemical formula of a molecular compound

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16
Q

diatomic molecule

A

a molecule containing only two atoms

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17
Q

interaction between charged particles in chemical bonds

A

approaching nuclei and electrons attract each other

2 nuclei repel each other

2 electron clouds repel each other

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18
Q

bond length

bond distance

A

distance between 2 bonded atoms at their minimum potential energy

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19
Q

bond energy

A

energy (in kJ⁄mol) required to break a chemical bond and form neutral isolated atoms

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20
Q

octet

A

4 pairs of electrons

8 electrons

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21
Q

octet rule

A

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

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22
Q

exceptions to the octet rule

A

hydrogen and helium are stable with 2 electrons (1 pair of electrons)

aluminum and boron are stable with 6 electrons (3 pairs of electrons)

some elements can be surrounded with more than 8 electrons when combined with highly electronegative elements

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23
Q

electron-dot notation

A

electron-configuration notation in which only the valence electrons of an atom of a particular element are indicated by dots placed around the element’s symbol

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24
Q

explanation of a Lewis structure

A

atomic symbols represent nuclei and inner-shell electrons

dot-pairs or dashes between two atomic symbols represent electron pairs in covalent bonds

dots adjacent to only one atomic symbol represent unshared electrons

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25
Q

unshared pair

lone pair

A

pair of electrons that is not involved in bonding and that belongs exclusively to 1 atom

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26
Q

structural formula

A

indicates the kind, number, arrangement, and bonds of atoms in a molecule

does not indicate the unshared pairs of atoms in a molecule

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27
Q

single bond

single covalent bond

A

covalent bond produced by sharing 1 pair of electrons between 2 atoms

represented by 2 dots in between 2 atoms’ atomic symbols or by 1 dash

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28
Q

multiple bonds

multiple covalent bonds

A

covalent bonds produced by sharing more than 1 pair of electrons between 2 atoms

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29
Q

types of multiple bonds

A

double bond

triple bond

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30
Q

double bond

double covalent bond

A

covalent bond produced by the sharing of 2 pairs of electrons between 2 atoms

represented by 2 side-by-side pairs of dots or by 2 parallel dashes

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31
Q

triple bond

triple covalent bond

A

covalent bond produced by the sharing of 3 pairs of electrons between 2 atoms

represented by 3 side-by-side pairs of dots or by 3 parallel dashes

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32
Q

determining factor of need for multiple bonds

A

satisfaction of the octet rule for each atom

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33
Q

resonance

A

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

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34
Q

covalently bonded networks

A

compounds which can be pictured as continuous 3-dimensional networks of bonded atoms

does not contain individual molecules

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35
Q

ionic compound

A

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

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36
Q

formula unit

A

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

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37
Q

crystal lattice

A

orderly arrangement of ions in an ionic compound which minimizes their potential energy

maximizes attraction and minimizes repulsions of ions

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38
Q

lattice energy

A

energy released when 1 mole of an ionic compound is formed

used to determine strength of ionic bonds

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39
Q

electrostatic forces

A

force that holds ions together in ionic compounds

very strong overall attraction between positive and negative charges

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40
Q

strength of forces of covalent bonding (in comparison to forces of ionic bonding)

A

very weak

41
Q

polyatomic ion

A

charged group of covalently bonded atoms

42
Q

delocalized electrons

sea of electrons

A

electrons that do not belong to any 1 atom

move freely about metal’s network of empty atomic orbitals

43
Q

metallic bond

A

chemical bond that results from the attraction between metal atoms and the surrounding delocalized electrons

does not result in the formation of a compound

44
Q

metallic bond strength

A

varies directly with nuclear charge of metal atoms and number of electrons in the metal’s electron sea

directly proportional to heat of vaporization

45
Q

metal’s heat of vaporization

A

amount of heat required to vaporize a metal

used to determine of strength of bonds

46
Q

molecular polarity

A

uneven distribution of molecular charge

determined by polarity of each bond with the geometry of the molecule

47
Q

VSEPR

A

valence-shell electron pair repulsion

48
Q

VSEPR theory

A

states that repulsion between the sets of valence-level electrons surrounding an atom causes these sets to be oriented as far apart as possible

useful for explaining the structure of molecules

helps to identify polarity of compounds

49
Q

hybridization

A

combination of 2 or more orbitals of similar energy in same atom

rearrangement of orbitals when an atom forms covalent bonds

causes an overall reduction of energy

50
Q

hybrid orbitals

A

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

51
Q

determining factor of number of hybrid orbitals

A

number of orbitals that have combined

52
Q

intermolecular forces

A

forces of attraction between molecules

53
Q

dipole

A

created by equal but opposite charges that are separated by a short distance

represented by an arrow with a head pointing toward the negative pole and a crossed tail situated at the positive pole

54
Q

direction of a dipole

A

from the dipole’s positive pole to its negative pole

55
Q

dipole-dipole force

A

intermolecular force between polar molecules

due to attraction of opposite dipoles of each molecule lining up

strong intermolecular force

56
Q

hydrogen bonding

A

type of dipole-dipole intermolecular force between a hydrogen atom and a highly electronegative atom

strongest intermolecular force

results in very high melting point and boiling point

usually represented by dotted lines connecting the hydrogen to the unshared electron pair of the electronegative atom

57
Q

London dispersion force

A

intermolecular force between nonpolar molecules

due to motion of electrons creating instantaneous poles on no polar molecules

very weak intermolecular force

results in very low melting point and boiling point

causes compounds to be gaseous at room temperature

58
Q

location of electrons in covalent bonds

A

overlapping orbitals

59
Q

resonance structure

A

a separate (though equally valid) electron dot notation of a molecule or polyatomic ion

60
Q

purpose of resonance structures

A

equalize bond lengths

create stronger bonds

61
Q

determining factor of need for resonance structures

A

presence of a double bond and a single bond on the same atom

62
Q

coordinate bond

dative covalent bond

A

covalently bonded pair of electrons which has been provided by only one of the bonding atoms

63
Q

sp3 hybridization

A

hybridization of 1 s orbitals and 3 p orbitals

forms no non-hybridized orbitals

oriented in a tetrahedral geometry

64
Q

sp2 hybridization

A

hybridization of 1 s orbital with 2 p orbitals

forms 1 non-hybridized orbital

oriented in a trigonal planar geometry

65
Q

sp hybridization

A

hybridization of 1 s orbital and 1 p orbital

forms 2 non-hybridized orbitals

oriented in a linear geometry

66
Q

linear geometry

A

molecular geometry of two or three atoms with bond angles of 180°

67
Q

general formulas of linear geometry

A

AB[E3]

AB2

68
Q

bent geometry

angular geometry

A

molecular geometry of three atoms with bond angles of 105°

69
Q

general formulas of bent geometry

general formulas of angular geometry

A

AB2[E]

AB2[E2]

70
Q

trigonal planar geometry

A

molecular geometry of four atoms with bond angles of 120°

71
Q

general formula of trigonal planar geometry

A

AB3

72
Q

tetrahedral geometry

A

molecular geometry of five atoms with bond angles of 109.5°

73
Q

general formula of tetrahedral geometry

A

AB4

74
Q

trigonal pyramidal geometry

A

molecular geometry of a five atoms with bond angles of 107°

75
Q

general formula of trigonal pyramidal geometry

A

AB3[E]

76
Q

trigonal bipyramidal geometry

A

molecular geometry of six atoms with bond angles of 120°

77
Q

general formula of trigonal bipyramidal geometry

A

AB5

78
Q

octahedral geometry

A

molecular geometry of seven atoms with bond angles of 90°

79
Q

general formula of octahedral geometry

A

AB6

80
Q

steps to determine molecular geometry for covalent compounds

A

draw electron dot diagram

determine polarity of bonds based on electronegativity difference of bonded atoms

count lone pairs on central atom

determine whether or not compound has symmetry

identify VSEPR shape

determine molecular polarity

81
Q

polarity of charged particles

A

no polarity

82
Q

state of ionic compounds

A

solid at room temperature

83
Q

melting point of ionic compounds

A

high

84
Q

boiling point of ionic compounds

A

high

85
Q

solubility in water of ionic compounds

A

soluble in water

86
Q

conductivity of ionic compounds

A

conductive of electricity in liquid state (or when dissolved in water)

87
Q

solubility in alcohol of ionic compounds

A

mostly insoluble in alchohol

88
Q

state of polar covalent compounds

A

solid, liquid, or gas at room temperature

89
Q

melting point of polar covalent compounds

A

low

90
Q

boiling point of polar covalent compounds

A

low

91
Q

solubility in water of polar covalent compounds

A

soluble in water

92
Q

conductivity of polar covalent compounds

A

possibly conductive of electricity

93
Q

solubility in alcohol of polar covalent compounds

A

possibly insoluble in alcohol

94
Q

state of nonpolar covalent compounds

A

mostly liquid or gas at room temperature

95
Q

melting point of nonpolar covalent compounds

A

low

96
Q

boiling point of nonpolar covalent compounds

A

low

97
Q

solubility in water of nonpolar covalent compounds

A

insoluble in water

98
Q

conductivity of nonpolar covalent compounds

A

not conductive of electricity

99
Q

solubility in alcohol of nonpolar covalent compounds

A

mostly soluble in alcohol

chemistry 1 (20 decks)

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