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CHEM 1127 Q > ch 4 - chemical bonding and molecular geometry > Flashcards

ch 4 - chemical bonding and molecular geometry Flashcards

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1
Q

NH4

A

ammonium; +1

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2
Q

OH

A

hydroxide; -1

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3
Q

NO3

A

nitrate; -1

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4
Q

NO2

A

nitrite; -1

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5
Q

ClO

A

hypochlorite; -1

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6
Q

ClO2

A

chlorite; -1

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7
Q

ClO3

A

chlorate; -1

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8
Q

ClO4

A

perchlorate; -1

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9
Q

MnO4

A

permanganate; -1

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10
Q

HCO3

A

hydrogen carbonate; -1

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11
Q

H2PO4

A

dihydrogen phosphate; -1

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12
Q

CO3

A

carbonate; -2

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13
Q

SO4

A

sulfate; -2

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14
Q

SO3

A

sulfite; -2

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15
Q

CrO4

A

chromate; -2

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16
Q

Cr2O7

A

dichromate; -2

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17
Q

HPO4

A

hydrogen phosphate; -2

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18
Q

PO4

A

phosphate; -3

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19
Q

binary acid

A

compound that contains hydrogen and one other element, bonded in a way that imparts acidic properties to the compound;
releases H+ ions in water

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20
Q

electronegativity

A

tendency of an atom to attract electrons in a bond to itself

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21
Q

formal charge

A

charge that would result on an atom by taking the number of valence electrons on the neutral atom and subtracting the nonbonding electrons and the number of bonds (1/2 the number of bonding electrons);

VE - LE - Bonds

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22
Q

hypervalent molecule

A

molecule containing at least one main group element that has more than eight electrons in its valence shell

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23
Q

ionic bond

A

strong electrostatic force of attraction between cations and anions in an ionic compound

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24
Q

Lewis structure

A

diagram showing lone pairs and bonding pairs of electrons in a molecule or an ion

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25
Q

octet rule

A

guideline stating that main group atoms will form structures in which eight valence electrons interact with each nucleus, counting bonding electrons as interacting with both atoms connected by the bond

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26
Q

oxyacid

A

compound that contains hydrogen, oxygen, and one other element, bonded in a way that imparts acidic properties to the covalent compound;
releases H+ ions when dissolved in water

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27
Q

pure covalent bond

A

covalent bonds between atoms of identical electronegativities

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28
Q

anion

A

negatively charged particle

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29
Q

cation

A

positively charged particle

30
Q

naming polyatomic ions

A

cation, anion, - ate

31
Q

naming monoatomic ions

A

cation, anion, -ide / metal, nonmetal, -ide

32
Q

naming a cation

A

-ide

33
Q

naming an anion*

A

anion cation

34
Q

numeric prefixes

A

only used for covalent bonds

35
Q

when pairing two nonmetals,

A

use numeric prefixes and put the least-metallic element last.

36
Q

binary acid

A

hydro - ic acid

37
Q

oxyacid

A

ate -> ic acid
ite -> ous acid

38
Q

bond dipole moment

A

separation of charge in a bond that depends on the difference in electronegativity and the bond distance represented by partial charges or a vector

39
Q

bond distance / length

A

distance between the nuclei of two bonded atoms

40
Q

covalent bond

A

formed when electrons are shared between atoms

41
Q

dipole moment

A

property of a molecule that describes the separation of charge determined by the sum of the individual bond moments based on the molecular structure

42
Q

electron-pair geometry

A

arrangement around a central atom of all regions of electron density

43
Q

electronegativity

A

tendency of an atom to attract electrons in a bond to itself

44
Q

formal charge

A

valence electrons - nonbonding electrons - bonds

45
Q

free radical

A

molecule that contains an odd number of electrons

46
Q

hypervalent molecule

A

molecule containing at least one main group element that has more than eight electrons in its valence shell

47
Q

inert pair effect

A

tendency of heavy atoms to form ions in which their valence s electrons are not lost

48
Q

ionic bond

A

strong electrostatic force of attraction between cations and anions in an ionic compound

49
Q

lone pair

A

two valence electrons that are not used to form a covalent bond

50
Q

molecular structure

A

arrangement of atoms in a molecule or ion;
structure that includes only the placement of the atoms in the molecule

51
Q

octahedral

A

a shape formed when a central atom has six areas of electron density; four groups form a square and the other two form the apex of pyramids

52
Q

polar covalent bond

A

covalent bond between atoms of different electronegativities

53
Q

polar molecule / dipole

A

molecule with an overall dipole movement

54
Q

pure covalent bond

A

covalent bond between atoms of identical electronegativities

55
Q

single bond

A

bond in which a single pair of electrons is shared between two atoms;
sigma bond

56
Q

tetrahedral

A

shape formed when a central atom has four areas of electron density; 109.5º angles between four corners

57
Q

trigonal pyramidal

A

shape formed when a central atom has three areas of electron density, with A at the apex

58
Q

trigonal planar

A

shape formed when a central atom has three areas of electron density; a flat triangle

59
Q

the further apart two atoms in the same period are,

A

the more polar their bond is

60
Q

ion

A

a molecule with a nonzero net charge due to gaining or losing electrons

61
Q

electron affinity

A

the energy change for the process of adding an electron to a gaseous atom to form an anion (negative ion);
increases across a period, decreases down a family

62
Q

binary compound

A

compound containing two different elements

63
Q

binary acid

A

compound that contains hydrogen and one other element, bonded in a way that imparts acidic properties to the compound

64
Q

oxyanion

A

an anion containing oxygen

65
Q

double / triple bond

A

covalent bond in which two / three pairs of electrons are shared between atoms;
pi bonds

66
Q

resonance

A

situation in which more than one Lewis structures can portray the bonding of atoms, and so the average of several is used instead

67
Q

VSEPR

A

valence-shell electron-pair repulsion theory;

theory used to predict bond angles in a molecule based on positioning regions of high electron density as far apart as possible to minimize electrostatic repulsion;

areas of electron density repel each other

68
Q

electron pair geometry

A

arrangement around a central atom of all regions of electron density

69
Q

molecular geometry

A

arrangement of atoms in a molecule or ion;
structure that includes only the placement of the atoms in a molecule

70
Q

covalent radii

A

radius generally decreases across a period and increases down a group

71
Q

ionization energy

A

energy required to remove a valence electron;
increases across a period, decreases down a family

CHEM 1127 Q (10 decks)

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