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chem 211 > ch 2 > Flashcards

ch 2 Flashcards

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1
Q

atom definition

A

the smallest individual complete unit of matter

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2
Q

element

A

matter made of only one type of atom

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3
Q

types of pure substances

A

elements
compounds

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4
Q

types of mixtures

A

homogenous
heterogenous

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5
Q

two categories of matter

A

pure substances
mixtures

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6
Q

types of compounds

A

ionic
covalent
organic
acids and bases

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7
Q

t or f : every compound is a pure substance

A

true

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8
Q

t or f: every compound contains two or more elements

A

true

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9
Q

t or f: every mixture contains two or more compounds

A

false

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10
Q

t or f: every pure substance is a compound

A

false

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11
Q

law of conservation of mass

A

The total mass of materials present after a chemical reaction is the same as the total mass present before the reaction. In other words, the number of atoms in the reactants must be equal to the number of atoms in the products.

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12
Q

law of definite proportions

A

Any given compound is composed of definite, constant proportions by mass of its elements.

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13
Q

law of constant composition

A

In a given compound, the relative numbers and kinds of atoms are constant

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14
Q

law of multiple proportions

A

If two elements (A & B) combine to form more than one compound, the elements must combine in ratios relative to the masses of individual A and B elements

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15
Q

JJ thompson experiment and discovery

A

discovery of the electron through the cathode ray experiment

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16
Q

robert millikan experiment

A

discovery of the charge of an electron through the oil drop experiment

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17
Q

dalton’s model of the atom consisted of

A

an indivisible sphere

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18
Q

thomson’s plum pudding model consisted of

A

negatively charged electrons suspended in a larger sphere of positive charge

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19
Q

ernest rutherford experiment and discovery

A

discovery of the basic model of the atom through the gold foil experiment

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20
Q

weighted average

A

sum of (% abundance in decimal form)(isotopic mass)

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21
Q

mass number

A

of protons and neutrons (not on the periodic table)

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22
Q

average atomic mass

A

weighted average mass of all isotopes of an element based on the number of protons, neutrons, and electrons
- value on the periodic table

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23
Q

nonmetals location of periodic table

A

to the right of the staircase

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24
Q

properties of metals

A

Solids at room temperature (except for Hg)
Shiny
Malleable
Ductile
Conduct heat and electricity well
Lose electrons to become cations
Participate in ionic and metallic bonding

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25
Q

properties of non metals

A

Many are gases at room temperature (some solids and liquids)
Solids are brittle
Conduct heat poorly
Conduct electricity poorly
Gain electrons to become anions
Participate in ionic and covalent bonding

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26
Q

elements in a group have

A

similar properties and trends

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27
Q

alkali metal properties

A
  • soft
  • metallic
  • found only in compounds
  • typical metallic properties
  • low density
  • low melting point
  • low ionization energy
28
Q

alkali metals react with water ____ and are even ___ reactive

A

violently; air

29
Q

alkaline earth metals properties

A
  • ## less air and water reactive
30
Q

reactivity tends to increase in what direction across the periodic table

A

down a group

31
Q

alkaline earth metals have higher ___ and __ ___ than alkali metals

A

densities; melting points

32
Q

chalcogens

A

group 6 (O, S, Se…)

33
Q

halogens are typical …

A

nonmetals

34
Q

halogen properties

A

highly negative electron affinities - exist as anions in nature

35
Q

halogens react directly with … to form …

A

metals; metal halides

36
Q

noble gas properties

A

colorless, odorless, mostly inert
large ionization energy
positive electron affinity
found as monoatomic gases

37
Q

ionic compound building block

A

formula unit

38
Q

covalent molecule building block

A

molecule

39
Q

acids are made of

A

non-metals, one of which is hydrogen

40
Q

diatomic elements

A

H2, N2, O2, F2, Cl2, Br2, I2 (BrINClHOF) (makes the number 7 on the periodic table

41
Q

naming binary covalent compounds

A
  • name first nonmetal as elemental name
  • add a prefix only if there is more than one
  • name second non metal replacing the ending with -ide
  • always use a prefix
42
Q

alkane skeletal formula

A

CxH2x+2

43
Q

organic prefixes 1-4

A

meth, eth, prop, but

44
Q

constitutional/structural isomers

A

Organic compounds with the same molecular formula but different atomic connectivity

45
Q

ionic compound structure

A

3D lattice
metal and nonmetal

46
Q

in ionic compounds, metals will always form ____ while nonmetals will always form ____

A

cations; anions

47
Q

zinc charge

A

2+

48
Q

Ag charge

A

1+

49
Q

Cd charge

A

2+

50
Q

which non-transition metals must always have roman numerals written next to them

A

Pb and Sn

51
Q

nitrate

A

NO3 -

52
Q

nitrite

A

NO2 -

53
Q

sulfate

A

SO4 -2

54
Q

sulfite

A

SO3 -2

55
Q

phosphate

A

PO4 -3

56
Q

carbonate

A

CO3 -2

57
Q

perchlorate

A

ClO4 -

58
Q

ammonium

A

NH4+

59
Q

hydroxide

A

OH-

60
Q

cyanide

A

CN-

61
Q

permanganate

A

MnO4 -

62
Q

acetate

A

CH3COO- or C2H3O2-

63
Q

chromate

A

CrO4 -2

64
Q

dichromate

A

Cr2O7 -2

65
Q

binary acids naming (protons and an element)

A
  • “hydro” for the hydrogen
  • replace ending of nonmetal with “ic”
  • add acid
66
Q

oxyacid (protons and a polyatomic ion) naming

A
  • say polyatomic ion name
  • if it ends in -ate replace with -ic
  • if it ends in -ite replace with -ous
  • add acid

chem 211 (4 decks)

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