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Chem > Ch.1-4 Early Alert and E1 > Flashcards

Ch.1-4 Early Alert and E1 Flashcards

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1
Q

States of Matter

A

solid, liquid, and gas

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2
Q

solid

A

closely packed

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3
Q

liquid

A

packed like a solid but can move, fixed volume but no fixed shape

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4
Q

gas

A

dispersed and free to move, has volume of shape on container

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5
Q

subsets of solid

A

crystalline and amorphous

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6
Q

crystalline

A

repeating order

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7
Q

amorphous

A

no order

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8
Q

the composition of matter is either…

A

a pure substance or mixture

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9
Q

2 categories of pure substance:

A

element or compound

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10
Q

element:

A

fundamental substance, cannot be seerated

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11
Q

compound

A

2 or more elements in fixed proportions, can be seperated

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12
Q

2 categories of a mixture

A

homogenous and heterogenous

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13
Q

homogenous

A

mixture has uniform composition, parts cannot be seen

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14
Q

heterogenous

A

mixture is not uniform and parts can be seen

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15
Q

physical properties

A

something a substance displays without changing its composition
-ex: smell, taste, color, melting point, density

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16
Q

chemical properties

A

something a substance displays by changing its composition through reaction
-ex: flammability, corrosiveness, acidity, and toxicity

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17
Q

The SI system

A

international system of measurements

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18
Q

length

A

meter

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19
Q

mass

A

kilogram

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20
Q

time

A

second

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21
Q

temperature

A

kelvin

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22
Q

amount of substance

A

mole

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23
Q

Mega (M)

A

6

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24
Q

kilo (k)

A

3

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25
Q

deci (d)

A

-1

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26
Q

centi (c)

A

-2

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27
Q

milli (m)

A

-3

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28
Q

micro (µ)

A

-6

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29
Q

ambiguous sig figs

A

no clear decimal point
1200

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30
Q

multiplication and division rule sig fig rule:

A

smallest amount of sig figs

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31
Q

addition and subtraction sig fig rule

A

fewest decimal places

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32
Q

F, C, and K temp scales

A

-C and K are the same size
C=(F-32)/1.8
K=C +273.15

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33
Q

D=

A

D= M/V

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34
Q

1ml=

A

1ml=1cm^3

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35
Q

mass laws that are the basis of modern atomic theory

A

mass of reaction= mass of product

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36
Q

Describe the experiments that led to the discovery of the electron and its charge

A

-cathode ray: experiment that led to the discovery that particles of the cathode have a negative charge
-glass tube with a cathode and an anode
and a pump. When charge was applied it
would be directed to the anode due to
being negatively charged
-charge to mass ration: experiment done to measure charge/ gram of an cathode ray particle
-these particles were named electrons

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37
Q

Explain the structure of an atom

A

-nucleus center with protons and neutrons and a surrounding orbit cloud which contain electrons

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38
Q

Describe the properties of subatomic particles and interpret isotope symbols

A

P+: positively charged and makes up most of the mass
N: neutral, makes up some of mass
e-: negatively charges, makes up no mass, in the surrounding cloud
Isotope symbols: above symbol is mass and below is atomic number (protons)

39
Q

elements combine to form __

A

compounds

40
Q

each element has its own ___

A

properties and characteristics

41
Q

mixture

A

elements can mix in any proportions
ex. H2, O2

42
Q

compound

A

elements are combined in fixed proportions
ex. H2O

43
Q

chemical bonds

A

-hold together compounds formed by atoms
-result from attractions between charged particles
-2 types: ionic and covalent

44
Q

ionic bond

A

-m and nm
-transfer of electrons

45
Q

covalent bond

A

-nm and nm
-sharing of electrons (sharing is Caring)

46
Q

in ionic bonds the metal becomes a __ and the nm becomes a __

A

-cation
-anion (because wants full octet)

47
Q

covalent bonds result in the creation of a ___

A

molecule

48
Q

the 3 types of chemical formulas

A

-empirical
-molecular
-structural

49
Q

empirical formula

A

-gives relative number of atoms of each element in a compound
ex. hydrogen peroxide: H2O2
ex. B2H6

50
Q

molecular formula

A

-gives actual number of atoms of each element
ex. hydrogen peroxide: GCF is 2 so HO
ex. B2H6 greatest common factor is 2 so BH3

51
Q

structural formula

A

-uses lines to represent covalent bonds and shows how atoms in a molecule are connected or bonded to each other

52
Q

the structural formula can also convey the molecules __

A

geometry

53
Q

molecular model

A

-more accurate and complete way to specify a compound
-many different types

54
Q

ball and stick molecular model

A

-atoms as balls and chemical bonds as sticks
-reflects the molecules shape
-the balls are typically color coded to specific elements

55
Q

space filling model

A

-atoms fill space between each other to closely represent a best estimate of its scaled size

56
Q

elements are either __ or __

A

-atomic
-molecular

57
Q

compounds are either __ or __

A

-molecular
-ionic

58
Q

atomic elements

A

-exist in nature with single atoms as their basic unit
-most elements

59
Q

molecular elements

A

-do not normally exist in nature
-single atoms as unit
-exist as molecules (2 or more atoms bonded together)

60
Q

molecular elements: diatomic

A

-2 atoms per molecule
-h2, N2, O2, F2, Cl2, Br2, i2
-only seven

61
Q

molecular elements: polyatomic

A

-P4, S8
-more than 2 atoms per molecule

62
Q

this type of element tends to form multiple types of charges and cannot be predicted

A

transition elements

63
Q

2 types of ionic compounds

A

1: metal forms only one type of ion
2: metal forms more that one type of ion, often transition metals

64
Q

ionic type 1 compound naming

A

cation (metal), base name of anion, +ide
ex. KCl: potassium chloride

64
Q

ionic type 2 compound naming

A

-name of cation (metal), charge of cation (roman numerals), base name of anion +-ide

65
Q

oxyanions

A

-oxygen and another element

66
Q

binary molecular compound naming

A

prefix, name of 1st element, prefix, base name of second +-ide

67
Q

acids

A

-molecular compounds that release H+ when dissolved in water

68
Q

2 types of acids

A

-binary acids (2 elements)
-oxyacids (oxygen)
-formula starts with H

69
Q

ate ->

A

ic

70
Q

-ite ->

A

ous

71
Q

hydrates

A

-ionic compounds containing a specific number of water molecules with each formula unit
-uses hydrate prefixes

72
Q

hemi

A

1/2

73
Q

mono

A

1

74
Q

di

A

2

75
Q

tri

A

3

76
Q

tetra

A

4

77
Q

penta

A

5

78
Q

hexa

A

6

79
Q

hepta

A

7

80
Q

octa

A

8

81
Q

molecular compound naming rules

A

-write name of element with smallest group first
-if same group write one with greatest row number first
-prefixes are given to each element to show number of atoms present

82
Q

nona

A

9

83
Q

deca

A

10

84
Q

naming binary acids

A

hydro, base name of nonmetal +ic, acid

85
Q

formula mass

A

entire mass of the compound

86
Q

composition of compounds/ mass percent composition

A

-how much of an element is in a compound
-mass percent of element X=)mass of element in 1 mole of compound/ mass of 1 mole of whole compound) x 100

87
Q

mass percent can be used as a …

A

-conversion factor
-Xg : 100g of compound

88
Q

finding the empirical formula

A

-convert percentages to g
-g to mol
-divide all by smallest
-multiply all by a number to get whole number

89
Q

finding molecular formula

A

-n=molar mass/empirical formula mass
-multiply empirical formula by n

90
Q

hydrocarbons

A

-contain only carbon and hydrogen

91
Q

when balancing chemical reactions start with…

A

the most complex substance

92
Q

percent yield=

A

actual/ theoretical x 100

93
Q

periodic law

A

elements with similar properties recur in a regular pattern

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