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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
what are the diatomic elements?
-hydrogen -nitrogen -oxygen -flourine -chlorine -bromine -iodine
26
solid to liquid
melting
27
liquid to gas
evaporation
28
gas to solid
depostion
29
liquid to solid
freezing
30
solid to gas
sublimation
31
gas to liquid
condensation
32
extensive vs. intensive physical properties
-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
33
chemical properties
-change that results in a different substance -ex. burning, rotting, tarnish, rusting, digesting
34
physical properties
-can be observed/measured without changing the identity of the substance -ex. cutting, grinding, freezing, melting, evaporating
35
desnity
-ratio of mass to volume in a substance -intensive d= m/v
36
accuracy
-closeness of measurements to correct value
37
precision
-closeness to measurements to each other
38
science
-the process of studying the natural world -search for knowledge
39
steps of scientific method
-state the problem -form a hypothesis -test hypothesis -record data -draw conclusions
40
branches of science
-life -physical -earth and space
41
life science examples
-anatomy -biology -genetics -ecology -zoology
42
physical science examples
-chemistry -physics
43
earth/space science examples
-geology -meteorology -atronomy
44
chemistry
-the study of the structure and properties of matter -study of changes matter undergoes -study of energy change associated
45
technology
-the application of science -making it useful
46
qualitiative vs. quantitative
-qualitative = qualities, using senses -ex. color, odor, texture, shape, size -quantitative= quantity, numerical values, measurements -ex. mass, density, temp, melting point, volume, length
47
independent variable
-variable that is changed
48
dependent variable
-variable that is observed -result of changing independent variable
49
hypothesis
-a possible explanation to a problem based on observation and research -must be testable
50
control
-element that remains unchanged by other variables -use it to compare
51
law vs. theory
-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
how to count sig figs
-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
scientific notation
-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
metric conversions
-kilo, hecto deka -base unit (meter, liter, gram) -deci, centi mili, ---, ---, micro, ---, ---, nano, angstrom
55
how far out to estimate
-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
mass base unit
kilogram (kg)
57
length base unit
meter (m)
58
time base unit
seconds (s)
59
temp base unit
kelvin (k)
60
amnt of substance base unit
mole (mol)
61
atomic number
-number of protons -determines the identity of an element -also number of electrons in a neutral atom
62
describe nuclear symbol
-mass number on top -atomic number on bottom -element symbol as big letter to the right
63
mass number
-protons plus neutrons -mass on periodic table rounded
64
hyphen notation
-mass number written after element name -ex. copper-65
65
protons
-positive charge -1 amu -in nucleus
66
neutrons
-neutral charge -1 amu -in nucleus
67
electrons
-negative charge -almost zero amu -orbit around nucleus
68
what makes up almost all the mass of the atom?
-nucleus (protons and neutrons)
69
what makes up almost all of the volume of the atom?
-the electron cloud/ orbit
70
how are atoms measured?
-angstrom (10^-10) -or picometers (10^-12)
71
what is the smallest atom?
-hydrogen
72
what is the average atomic mass?
-below element symbol on periodic table -average of all isotopes
73
ion
-charged atom -there are anions or cations -formed by gaining or losing electrons
74
anion
-negative ion -formed by gaining electrons
75
cation
-positive ion -formed by gaining electrons
76
valence electrons
-outer shell electrons -involved in bonding
77
list the groups numbers of electrons on the periodic table
-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
what is the most ve- and element can have?
-8 -this makes a full outer ring -"octet"
79
group 1 on the periodic table
-alkali metals -1 ve- -most reactive metals -soft -silvery in clor -never form in nature
80
group 2 on the periodic table
-alkaline earth metals -2 ve- -less reactive than alkali metals but still reactive -never form in nature -alkaline means basic
81
groups 3- 12 on the periodic table
-transition metals -have typical metal properties
82
group 17 on the periodic table
-halogens -7 ve- -most reactive nonmetals -only found in pure form as diatomic elements
83
group 18 on the periodic table
-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
how is the periodic table organized?
-by atomic number -groups are up and down -periods are side to side
85
metals
-readily lose electrons to form cations -ductile -malleable -good conductors -luster -form alloys -mostly solids at room temp
86
which metal is not a solid at room temp?
-mercury
87
metalloids
-zig zag on the periodic table from aluminum to antimony -form both anions and cations -between a metal and a nonmetal -semi conductors
88
nonmetals
-readily gain electrons to form anions -not ductile or malleable -bad conductors -brittle when solid -some are gases -1 liquid
89
which nonmetal is a liquid at room temp?
-bromine
90
lanthanides
-at the bottom on the top -elements 77-71 -rare earth metals
91
actinides
-at the bottom on the bottom -elements 89-103 -radioactive
92
democritus
-"atomos" -greek philosopher -matter is made up of indivisable particles called atomos
93
dalton
-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
jj thomson
-plum pudding model -discovered electron
95
rutherford
-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
bohr
-rings model -electrons orbit nucleus in fixed paths called orbits
97
quantum mechanical model
-many scientists -mathematically describes wave properties of electrons -positive nucleus iwth cloud of electrons -electrons act as waves and particles
98
which parts of dalton's theory were proved untrue and how?
-atoms cannot divide, be created, or destroyed -nuclear chemistry/ nuclear bomb -atoms of an element are identical -isotopes
99
timeline of models of the atom
-democritus/dalton billiard ball -thomson plum pudding -rutherford -bohr -quantum mechanics
100
percent error formula
-real value- value you got divided by real value times 100

chemistry (10 decks)

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