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chemistry > midterm > Flashcards

midterm Flashcards

1
Q

what is the emergency equpiment in the lab?

A

-exit door
-eye wash station
-fire exinguisher
-saftey shower
-fire blanket
-first aid kit

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2
Q

matter

A

-anything that has mass and volume

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3
Q

volume

A

-amount of three dimensional space an object takes up

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4
Q

mass

A

-measure of amount of matter

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5
Q

atom

A

-small unit of an element that maintains its chemical identity

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6
Q

element

A

-pur substance
-cannot be broken down into simpler, stable substances
-is made of 1 type of atom

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7
Q

kinetic molecular theory of matter

A

-all matter is composed of particles that are always moving
-particles have space between them
-more energy = more space
-all particles have energy
-temperature is the measure of the average kinetic energy of particles
-if you change the temperature a change in state may occur
-attractive forces between particles are stronger as particles are closer together

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8
Q

characteristics of a solid

A

-definite shape and volume
-particles packed close together
-particles vibrate in a fixed motion
-strong attractive forces
-low energy

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9
Q

characteristics of a liquid

A

-definite volume but not shape
-particles are somewhat close together but can slide past each other
-particles flow past each other
-strong attractive forces
-medium energy

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10
Q

characteristics of a gas

A

-no definite shape or volume
-particles are spaced out
-particles move with great speed
-weak attractive forces
-high energy

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11
Q

pure substance

A

-fixed composition
-composed of only one type of particle

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12
Q

what are the 2 types of pure substances?

A

-compounds
-elements

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13
Q

what are the 2 types of pure substances made of?

A

-elements are made of atoms
-compounds are made of molecules or ions

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14
Q

mixture

A

-physical combination of two or more substances
-identities and properties of the substances are indivdually retained
-can be separated by physical means

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15
Q

mixture vs. compound

A

-compounds have a definite composition
-mixtures don’t, their composition varies

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16
Q

heterogeneous mixture

A

-not the same throughout
-particles are large enough to see
-not uniform
-ex. oil and water

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17
Q

homogeneous mixture

A

-appears the same throughout
-particles don’t settle out when left standing
-aka a solution
-ex. saltwater

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18
Q

what are the different separation techniques?

A

-filtration
-evaporation
-distillation
-decanting
-chromatography

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19
Q

filtration

A

-passing a mixture through a filter
-uses property of size

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20
Q

evaporation

A

-letting a mixture evaporate
-uses the property of vaporization point
-ex. saltwater

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21
Q

distillation

A

-separates liquid mixtures
-liquid with lowest boiling point vaporizes first
-collect vapor and condense as pure liquid
-uses property of vaporization point

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22
Q

evaporation vs. distillation

A

-evaporation is concerned with collecting the solid
-distillation wants the pure liquid that is vaporized

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23
Q

decanting

A

-separation by pouring off the liquid layer and leaving solids behind
-uses property of state of matter

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24
Q

chromatography

A

-separates based on attraction
-ex. hydrophobic

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25
Q

what are the diatomic elements?

A

-hydrogen
-nitrogen
-oxygen
-flourine
-chlorine
-bromine
-iodine

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26
Q

solid to liquid

A

melting

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27
Q

liquid to gas

A

evaporation

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28
Q

gas to solid

A

depostion

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29
Q

liquid to solid

A

freezing

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30
Q

solid to gas

A

sublimation

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31
Q

gas to liquid

A

condensation

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32
Q

extensive vs. intensive physical properties

A

-extensive depends on amount of matter present
-ex. mass and volume
-intensive does not depend on matter present
ex. color, density, boiling point, malleability, ductility

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33
Q

chemical properties

A

-change that results in a different substance
-ex. burning, rotting, tarnish, rusting, digesting

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34
Q

physical properties

A

-can be observed/measured without changing the identity of the substance
-ex. cutting, grinding, freezing, melting, evaporating

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35
Q

desnity

A

-ratio of mass to volume in a substance
-intensive
d= m/v

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36
Q

accuracy

A

-closeness of measurements to correct value

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37
Q

precision

A

-closeness to measurements to each other

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38
Q

science

A

-the process of studying the natural world
-search for knowledge

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39
Q

steps of scientific method

A

-state the problem
-form a hypothesis
-test hypothesis
-record data
-draw conclusions

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40
Q

branches of science

A

-life
-physical
-earth and space

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41
Q

life science examples

A

-anatomy
-biology
-genetics
-ecology
-zoology

42
Q

physical science examples

A

-chemistry
-physics

43
Q

earth/space science examples

A

-geology
-meteorology
-atronomy

44
Q

chemistry

A

-the study of the structure and properties of matter
-study of changes matter undergoes
-study of energy change associated

45
Q

technology

A

-the application of science
-making it useful

46
Q

qualitiative vs. quantitative

A

-qualitative = qualities, using senses
-ex. color, odor, texture, shape, size
-quantitative= quantity, numerical values, measurements
-ex. mass, density, temp, melting point, volume, length

47
Q

independent variable

A

-variable that is changed

48
Q

dependent variable

A

-variable that is observed
-result of changing independent variable

49
Q

hypothesis

A

-a possible explanation to a problem based on observation and research
-must be testable

50
Q

control

A

-element that remains unchanged by other variables
-use it to compare

51
Q

law vs. theory

A

-theory is an explanation based on hypothesis, observation, and testing
-answers how and why
-law is a statment about the natural world
-predicts what will occur in a given set of conditions
-answers what happens without explaining how or why

52
Q

how to count sig figs

A

-0’s dont count unless they are embedded or there is a decimal
-ex. 203,000 has 3 sig figs
-if there were a line above one of the zeros it would stop there
-ex. 203,000. has 6 sig figs
-ex. 0.00570 has 3 sig figs
-ex. 2.800 has 4 sig figs

53
Q

scientific notation

A

-represents really small or really big numbers
-ex. 32,000 is 3.2 x 10^4
-ex. 0.000032 is 3.2 x 10^-5

54
Q

metric conversions

A

-kilo, hecto deka
-base unit (meter, liter, gram)
-deci, centi mili, —, —, micro, —, —, nano, angstrom

55
Q

how far out to estimate

A

-add one decimal place/ place from the values it is in between
-ex. between 23 and 24 closer to 24 you would say 24.6

56
Q

mass base unit

A

kilogram (kg)

57
Q

length base unit

A

meter (m)

58
Q

time base unit

A

seconds (s)

59
Q

temp base unit

A

kelvin (k)

60
Q

amnt of substance base unit

A

mole (mol)

61
Q

atomic number

A

-number of protons
-determines the identity of an element
-also number of electrons in a neutral atom

62
Q

describe nuclear symbol

A

-mass number on top
-atomic number on bottom
-element symbol as big letter to the right

63
Q

mass number

A

-protons plus neutrons
-mass on periodic table rounded

64
Q

hyphen notation

A

-mass number written after element name
-ex. copper-65

65
Q

protons

A

-positive charge
-1 amu
-in nucleus

66
Q

neutrons

A

-neutral charge
-1 amu
-in nucleus

67
Q

electrons

A

-negative charge
-almost zero amu
-orbit around nucleus

68
Q

what makes up almost all the mass of the atom?

A

-nucleus (protons and neutrons)

69
Q

what makes up almost all of the volume of the atom?

A

-the electron cloud/ orbit

70
Q

how are atoms measured?

A

-angstrom (10^-10)
-or picometers (10^-12)

71
Q

what is the smallest atom?

A

-hydrogen

72
Q

what is the average atomic mass?

A

-below element symbol on periodic table
-average of all isotopes

73
Q

ion

A

-charged atom
-there are anions or cations
-formed by gaining or losing electrons

74
Q

anion

A

-negative ion
-formed by gaining electrons

75
Q

cation

A

-positive ion
-formed by gaining electrons

76
Q

valence electrons

A

-outer shell electrons
-involved in bonding

77
Q

list the groups numbers of electrons on the periodic table

A

-group 1 has 1
-group 2 has 2
-group 13 has 3
-group 14 has 4
-group 15 has 5
-group 16 has 6
-group 17 has 7
-group 18 has 8

78
Q

what is the most ve- and element can have?

A

-8
-this makes a full outer ring
-“octet”

79
Q

group 1 on the periodic table

A

-alkali metals
-1 ve-
-most reactive metals
-soft
-silvery in clor
-never form in nature

80
Q

group 2 on the periodic table

A

-alkaline earth metals
-2 ve-
-less reactive than alkali metals but still reactive
-never form in nature
-alkaline means basic

81
Q

groups 3- 12 on the periodic table

A

-transition metals
-have typical metal properties

82
Q

group 17 on the periodic table

A

-halogens
-7 ve-
-most reactive nonmetals
-only found in pure form as diatomic elements

83
Q

group 18 on the periodic table

A

-noble gases
-8 ve- (except helium 2 ve- equals full ring)
-unreactive aka inert
-colorless, odorless gases
-only found in pure form in nature

84
Q

how is the periodic table organized?

A

-by atomic number
-groups are up and down
-periods are side to side

85
Q

metals

A

-readily lose electrons to form cations
-ductile
-malleable
-good conductors
-luster
-form alloys
-mostly solids at room temp

86
Q

which metal is not a solid at room temp?

A

-mercury

87
Q

metalloids

A

-zig zag on the periodic table from aluminum to antimony
-form both anions and cations
-between a metal and a nonmetal
-semi conductors

88
Q

nonmetals

A

-readily gain electrons to form anions
-not ductile or malleable
-bad conductors
-brittle when solid
-some are gases
-1 liquid

89
Q

which nonmetal is a liquid at room temp?

A

-bromine

90
Q

lanthanides

A

-at the bottom on the top
-elements 77-71
-rare earth metals

91
Q

actinides

A

-at the bottom on the bottom
-elements 89-103
-radioactive

92
Q

democritus

A

-“atomos”
-greek philosopher
-matter is made up of indivisable particles called atomos

93
Q

dalton

A

-billiard ball model
-all matter is composed of atoms
-atoms of a given element are identical
-atoms cannot divide, be created, or destroyed
-atoms of different elements combine to make compounds
-atoms are separated, rearranged, or combined in chemical reactions

94
Q

jj thomson

A

-plum pudding model
-discovered electron

95
Q

rutherford

A

-star looking model
-gold foil experiement
-used alpha particles and shot them through gold foil
-most passed through but some bounced back
-concluded that the atom is mostly empty space with a dense, small, positively charged nucleus

96
Q

bohr

A

-rings model
-electrons orbit nucleus in fixed paths called orbits

97
Q

quantum mechanical model

A

-many scientists
-mathematically describes wave properties of electrons
-positive nucleus iwth cloud of electrons
-electrons act as waves and particles

98
Q

which parts of dalton’s theory were proved untrue and how?

A

-atoms cannot divide, be created, or destroyed
-nuclear chemistry/ nuclear bomb
-atoms of an element are identical
-isotopes

99
Q

timeline of models of the atom

A

-democritus/dalton billiard ball
-thomson plum pudding
-rutherford
-bohr
-quantum mechanics

100
Q

percent error formula

A

-real value- value you got divided by real value times 100

chemistry (10 decks)

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