Chemistry-Ch. 1-2

Front 1

John Dalton
1. where
2. when
3. what did he do/say

Back 1

1. Brit
2. 1766-1844
3. atomic theory of matter-->the basis of modern chem

Front 2

law vs. hypothesis vs. theory

Back 2

law=statement/equation abouta relationship or regularity of nature
hypothesis=tentative explanation of some regularity f nature
theory=tested explanation of basic natural phenomena

Front 3

law of conservation of mass
1. definition
2. who
3. significance

Back 3

1. total mass remains constant during a chem change/reaction
2. Antoine Lavoisier (Fr.)
3. a)used to clarify phenomenon of combustion/burning
b)a burnt material chem combines w/ a component of air (O)

Front 4

equation of force of gravity

Back 4

F = G * m1 * m2 / r^2
F-force of gravity
G-gravitational constant
m1&m2-the 2 masses
r-distance between the 2 objects

Front 5

Explain:
mercury + oxygen -->mercury(II) oxide

Back 5

mercury combines with oxygen and forms a red-orange substance when it burns (ie combines with oxygen)

Front 6

What distinguish gases, liquids, and solids from one another? (2 answers)

Back 6

1. rigidity
2. compressibility/expansibility

Front 7

Define:
1. physical change
2. chemical change/reaction
3. physical property
4. chemical property

Back 7

1. change in form of matter but NOT chem identity
2. change in which 1/more kinds of matter transform into new matter(s)
3. propoerty that can be observed without changing chem identity
4. property involving a chem change

Front 8

outline the relationships among elements, compounds, mixtures, substances, and matter

Back 8

MATTER
-->SUBSATNCES and MIXTURES
-SUBSTANCE:matter that can't be separated into other kinds of matter by physical processes
==>ELEMENTS AND COMPOUNDS
-element: substance that can't be decomposed into simpler substances by any chem reaction
-compound: chem combined elements
-MIXTURE: material that can be separated by physical means into 2/more substances
==>HOMOGENEOUS AND HETEROGENEOUS MIXTURES
-homogeneous mixture: aka solution; uniform in its properties
-heterogeneous mixture: physically distinct parts

Front 9

chromatography (def)

Back 9

group of similar separation techniques
1. paper chromatogrpahy-line of ink drawn along lower edge of paper and dyes of ink separate as a solution of methanol and h2o
2. column chromatography:
a)pour solution into top of column containing chalk
b) add pure liquid to column
c)collect each substance in a separate flask
3. gas chromatography

Front 10

significant figures
1. definition
2. 3 rules for how to count significant numbers

Back 10

1. digits that include all certain digits plus one uncertain digit
2. a)zeros at beginning of number don't count as significant numbers
b)terminal zeros ending at right of decimal point are significant

Front 11

SI base units (quantity, unit, symbol)
1. length
2. mass
3. time
4. temp
5. amount of substance
6. electric current
7. luminous intensity

Back 11

1.meter-m
2.kilogram-kg
3.second-s
4.kelvin-K
5.mole-mol
6.ampere-A
7.candela-cd

Front 12

1 kg=??? lbs

Back 12

1 kg=2.2 lbs

Front 13

SI prefixes (10)
(include multiple, prefix, and symbol)

Back 13

mega-M-10^6
kilo-k-10^3
hecto-h-10^2
deka-da-10^1
deci-d-10^-1
centi-c-10^-2
milli-m-10^-3
micro-u-10^-6
nano-n-10^-9
pico-p-10^-12

Front 14

temperature
-boiling point
-room temperature
-freezing point
-formulas for conversion
formulas

Back 14

-boiling point: 373 K, 100 C, 212 F
-room temp: 293 K, 20 C, 68 F
-freezing point: 273 K, 0 C, 32 F
-C<->K:
TK=(tC*[1K/1 C])+273.15 K
-F<->C
tC=5C/9F*(tF-32 F)

Front 15

In what unit(s) do you measure volume?

Back 15

m^3, cm^3(ie cc), liter(L)/dm^3

Front 16

derived units: (quantity, def of quantity, SI unit)
1. area
2. volume
3. density
4. speed
5. acceleration
6. force
7. pressure
8. energy

Back 16

1. length^2,m^2
2. length^3,m^3
3. mass per unit volume, kg/m^3
4. dist traveled per unit time, m/s
5. speed changed per unit time, m/s^2
6. mass times acceleration, kg*(m/s^2) (=newton/N)
7. force per unit area, kg/(m*s^2) (=pascal/Pa)
8. force times distance traveled, kg*(m^2/s^2)

Front 17

density def and formula

Back 17

density=mass/volume
uses of density:
-identify a substance
-determine purity of a substance

Front 18

dimensional analysis definition

Back 18

aka factor-label method
-method of calculation in which one carries the units for quantities

Front 19

atomic theory of matter

Back 19

1. all matter has atoms
2.elements have only one kind of atom
3.a compound is matter w/ atoms of 2/more elements chem combined in fixed proportions
4. chem reaction rearranges atoms in reacting substances to give new chem combos