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general chemistry > chapter 6 > Flashcards

chapter 6 Flashcards

1
Q

what is the octet rule?

A

tendency of atoms to attain a stable e- configuration
(NOT USED W/ TRANSITION ELEMENTS)

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2
Q

what is an ionic bond?

A

ve- of metal atoms are transferred to nonmetal atoms
ex: NA stoms lose e- and Cl gains the e- to form NaCl

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3
Q

what are covalent bonds?

A

nonmetal atoms share ve-
ex:H2O -> H shares the e- with H

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4
Q

what are ions?

A

form when atoms lose or gain e- to form a stable e- configuration

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5
Q

what are ionic compounds?

A

1+ e- are transferred from metals–>nonmetals which form positive and negative ions

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6
Q

elements on the left side (and in group 3A) ___ e- to form a stable configuration

A

LOSE (form + charge)

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7
Q

elements on the right side ___ e- to form a stable configuration

A

GAIN (form - charge)

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8
Q

what are chemical formulas?

A

represent the symbols + subscripts in the lowest whole # ratio of the atoms or ions
i.e total amt. of positive charge = total amt. of negative charge

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9
Q

what is a formula unit?

A

lowest ratio of ions

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10
Q

what is the formula for HYDROXIDE?

A

OH-

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11
Q

what is the formula for AMMONIUM?

A

NH4+

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12
Q

what is the formula for NITRATE?

A

NO3-

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13
Q

what is the formula for NITRITE?

A

NO2-

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14
Q

what is the formula for PERCHLORATE?

A

ClO4-

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15
Q

what is the formula for CHLORATE?

A

ClO3-

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16
Q

what is the formula for CHLORITE?

A

ClO2-

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17
Q

what is the formula for HYPOCHLORITE?

A

ClO-

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18
Q

what is the formula for CARBONATE?

A

CO3 2-

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19
Q

what is the formula for HYDROGEN CARBONATE (aka bicarbonate)

A

HCO3-

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20
Q

what is the formula for CYANIDE?

A

CN-

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21
Q

what is the formula for ACETATE?

A

C2H3O2-

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22
Q

what is the formula for SULFATE?

A

SO4 2-

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23
Q

what is the formula for HYDROGEN SULFATE? (aka bisulfate)

A

HSO4-

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24
Q

what is the formula SULFITE?

A

SO3-

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25
Q

what is the formula for HYDROGEN SULFITE? (aka bisulfite)

A

HSO3-

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26
Q

what is the formula for PHOSPHATE?

A

PO4 3-

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27
Q

what is the formula for HYDROGEN SULFATE?

A

HPO4 2-

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28
Q

what is the formula for DIHYDROGEN PHOSPHATE?

A

H2PO4 2-

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29
Q

what is the formula for PHOSPHITE?

A

PO3 3-

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30
Q

what is happening when the prefixes go from per -> -ate -> -ite -> hypo?

A

losing an oxygen

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31
Q

what is happening when the prefixes go from hypo -> -ite -> -ate -> per-?

A

gaining an oxygen

32
Q

how many oxygens are typically in something that ends in -ite?

33
Q

how many oxygens are typically in something that ends -ate?

34
Q

how many oxygens are typically in something that begins with hypo-?

35
Q

how many oxygens are typically in something that begins with per-?

36
Q

what are polyatomic ions?

A

group of covalently bonded atoms that has an overall charge

37
Q

what is a molecular compound?

A

atoms of 2+ nonmetals that share 1+ ve-
held together by a covalent bond (b/w 2 nonmetals)

38
Q

what are molecules?

A

discrete groups of atoms in a definite proportion

39
Q

prefix for 1?

40
Q

prefix for 2?

41
Q

prefix for 3?

42
Q

prefix for 4?

43
Q

prefix for 5?

44
Q

prefix for 6?

45
Q

prefix for 7?

46
Q

prefix for 8?

47
Q

prefix for 9?

48
Q

prefix for 10?

49
Q

when is an ionic bond formed?

A

metal + nonmetal

50
Q

when is a molecular bond formed?

A

nonmetal + nonmetal

51
Q

what is a bonding pair?

A

shared e-s
2 dots or a single line b/w atoms

52
Q

what is a lone pair?

A

nonbonding pairs
placed outside of an atom (rep as dots)

53
Q

what are diatomic atoms?

A

contain 2 like atoms (natural state of some)

54
Q

what are examples of diatomic atoms?

A

N2, O2, F2, Cl2, Br2, I2, H2

55
Q

what is a double bond?

A

when 2 pairs of e- are shared b/w 2 atoms

56
Q

what is a triple bond?

A

when 3 pairs of e- are shared b/w 2 atoms

57
Q

what factor determines which atom is the central atom?

A

whichever atom has the highest bonding capacity
typically C -> O -> N

58
Q

what is electronegativity?

A

ability to attract the shared e- in a chemical bond
nonmetals have higher e-neg. bcz they have a higher e- attraction

59
Q

what is a NONpolar covalent bond?

A

covalent bonds b/w atoms w/ IDENTICAL or V. SIMILAR e-neg. values

60
Q

what are the e-neg. difference values for a nonpolar covalent bond?

61
Q

what are polar covalent bonds?

A

covalent bonds b/w atoms with DIFFERENT e-neg. values
i.e e- shared unequally -> attracted to the more e-neg. atom

62
Q

what are the e-neg. difference values for a polar covalent bond?

63
Q

what is a dipole?

A

polar covalent bond that has a separation of charges + indicated by µ+ or µ-
also rep. by an arrow pointing to the more e-neg. atom

64
Q

when do dipoles occur?

A

typically in covalent bonds containing N, O, or F

65
Q

what is the valence shell e- pair repulsion theory?

A

e- groups are arranged as far a part as possible around the central atoms to minimize repulsion (atoms saying “ew” to atoms of like charges)

66
Q

which elements are exceptions to the octet rule?

A

Sulfur, Boron, Beryllium, and Hydrogen

67
Q

how many e- can surround Boron?

A

6 (form 3 bonds)

68
Q

how many e- can surround Hydrogen?

A

2 (forms 1 bond)

69
Q

how many e- can surround Sulfur?

A

10 (forms 5 bonds)

70
Q

how many e- can surround Beryllium?

A

4 (forms 2 bonds)

71
Q

what are the e-neg. difference values for ionic bonds

72
Q

what is a nonpolar molecule?

A

all bonds are nonpolar OR all polar molecules cancel eachother out (dipoles point in opposite directions)

73
Q

what is a polar molecule?

A

one end of the molecule is more negatively charged than the other end

74
Q

what are dipole-dipole attractions?

A

(occur in polar molecules) intermolecular forces occur b/w the positive end of one molecule + the negative end of another

75
Q

what is a hydrogen bond?

A

occurs b/w partially pos. hydrogen atom in one molecule + the partially neg. F/O/N
*strongest type of IMF b/w polar covalent molecules

76
Q

what is a dipersion force?

A

very weak attraction + only IMF that occur b/w NONpolar molecules

77
Q

what is a temporary dipole?

A

when movement of the e- (which are normally =ly distributed) may place more of them in one part of the molecule
align the molecules so that the pos. end of one molecule = attracted to the neg. end of another molecule

general chemistry (4 decks)

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