10Th Grade Chemistry

Front 1

definition of Matter

Back 1

anything that has mass or occupies space

Front 2

5 areas of Chemistry

Back 2

Biochemistry
Organic
Inorganic
Analytical
Physical

Front 3

definition of Biochemistry

Back 3

process that takes place in organisms

Front 4

def of Organic

Back 4

living things that contain carbon

Front 5

def of Inorganic

Back 5

nonliving things that don’t contain carbon

Front 6

def of Analytical

Back 6

analyzing composition of matter

Front 7

def of Physical

Back 7

rate of which something happens/process

Front 8

def of Pure chemistry

Back 8

pursuit of chemical knowledge

Front 9

def of Applied chemistry

Back 9

research directed for practical goal

Front 10

def of Extensive properties

Back 10

depends on amount of matter that is present (quantity)

Front 11

examples of Extensive properties

Back 11

Mass, volume, energy

Front 12

def of Intensive properties

Back 12

does not depend on the amount of matter present (quality);

Front 13

examples of Intensive properties

Back 13

Density, melting point, boiling point

Front 14

def of physical properties

Back 14

substance where the quality changes but doesn’t change with another substance

Front 15

def of Chemical properties

Back 15

shows when a substance changes into or interacts with another substance

Front 16

def of Substance

Back 16

type of matter that has a defined fixed composition

Front 17

How to tell when chemical change occurs

Back 17

-gas being formed
-changing appearance
-changes into solid/precipitate

Front 18

def of Mixture

Back 18

-combination of different substances
-can physically separate it
-ex. Air, Foods

Front 19

def of Compound

Back 19

can’t physically separate it

Front 20

def of Heterogeneous mixture:
and examples

Back 20

-one or more visible boundaries between the compounds
-ex: bowl of apples and pears, or sand in water

Front 21

def of Homogeneous mixture
and examples

Back 21

-has no visible boundaries, component are mixed individual atoms, ions and molecules
-ex. Salt water and air (can’t physically separate it)

Front 22

def of Pure substances

Back 22

-can’t be decomposed by chemical means like elements- gold aluminum
-can be like compounds

Front 23

5 Basic separation techniques

Back 23

Fltration
Crystalization
Distillation
Extraction
Chromatology

Front 24

def of Filtration

Back 24

-separates components of a mixture based upon differences in particle size.

Front 25

def of Crystallization

Back 25

-separation based on differences in solubility (able to mix) of components in a mixture

Front 26

def of Distillation

Back 26

-separation based up on differences in volatility (evaporate)

Front 27

def of Extraction

Back 27

-separation is based upon differences in solubility in different solvents (major material)

Front 28

def of Chromatography

Back 28

-separation based upon differences in solubility in a solvent versus a stationary phase

Front 29

def of Element

Back 29

-simplest form of matter (oxygen or hydrogen);

Front 30

def of Compounds

Back 30

-substance that contains two or more elements chemically combined; has a fixed proportion

Front 31

def of Physical methods
and examples

Back 31

-can’t break compounds
-ex. boil water doesn’t make oxygen and hydrogen

Front 32

things that make a chemical change

Back 32

-Burn, rot, rust, decompose, ferment, explode, or corrode means a chemical change

Front 33

-substance present is the...
-substance produced is the...

Back 33

-reactant
-product

Front 34

Chemical change involves...

Back 34

transfer of energy

Front 35

def or Law of conservation of mass

Back 35

-physical/chemical change mass conserves
-not created nor destroyed

Front 36

the def of Atom

Back 36

-the smallest unit of an element, building blocks of matter

Front 37

the def of Element

Back 37

-pure substance made up of one kind of atom

Front 38

the def of Compound

Back 38

-substance that is made from the two or more elements that are chemically bounded

Front 39

Phlogiston Theory is...

Back 39

-Combustible materials contained phlogiston- released when burning
-air attracted phlogiston, burning stopped when air became “saturated”
-had negative mass

Front 40

Antoine Lavoisier found out...

Back 40

-proved oxygen in air necessary for burning

Front 41

def of Measurement

Back 41

-quantitative observation consisting of number and a unit

Front 42

def of Uncertainty measurement

Back 42

-a digit that must be estimated is the uncertain digit

Front 43

def of Precision

Back 43

-refers to degree of agreement over several measurements made in same manner

Front 44

def of Accuracy

Back 44

-agreement of a particular value with the true value

Front 45

def of Random error

Back 45

-the numbers have no pattern

Front 46

def of Systematic error

Back 46

numbers are in a pattern

Front 47

When there’s a decimal and sig figs

Back 47

-start counting sig figs after zeros after the decimal

Front 48

sig figs and exact numbers

Back 48

Exact numbers have infinite number of sig figs

Front 49

When there isn’t a decimal present and sig figs

Back 49

-don’t count ending zeros

Front 50

sig figs in Multiplying or Dividing

Back 50

-number of sig figs in answer = least number of sig figs in calculations

Front 51

sig figs in Adding or Subtracting

Back 51

-number of decimal places in result= places in least precise measurement

Front 52

International System of Units of
Length
Mass
Temp
Time
Amt. Sub
Electric current

Back 52

-meter
-kilogram
-kelvin
-second
-mole
-ampere

Front 53

--Metric prefixes-
kilo
deci
centi
milli

Back 53

-1000 times larger (k)
-10 times smaller (d)
-100 times smaller (c)
-1000 times smaller (m)

Front 54

Kelvin is
conversion

Back 54

the absolute temperature scale begins at absolute Zero; only has pos. values
-K= celcius + 273.15