Chem

Front 1

chemistry

Back 1

The study of the properties and
transformations of matter.

Front 2

matter

Back 2

Anything that has mass and occupies space –
things you can see, touch, taste, or smell.

Front 3

property

Back 3

characteristic that can be used to describe a
substance. Size, color, temperature are most familiar
properties of matter. Less familiar properties include:
• Chemical composition: what matter is made of.
• Chemical reactivity: how matters behave.

Front 4

physical change

Back 4

Does not alter the
chemical makeup of a substance. Change is
reversible. Melting of solid ice is a physical
change. In this case only change in form
takes place and the change is reversible.

Front 5

chemical change

Back 5

Alters chemical makeup
of a substance. Change is irreversible.
Rusting of iron is a chemical change. Here,
iron combines with oxygen and produces a
new substance rust.

Front 6

– Gas

Back 6

:A substance that has neither a definite
volume nor a definite shape.

Front 7

– Liquid:

Back 7

A substance that has a definite volume but that changes shape to fill the container.

Front 8

Solid:

Back 8

A substance that has a definite shape and volume.

Front 9

Pure Substance:

Back 9

Uniform in its chemical composition
and properties. Sugar and water are pure substances.

Front 10

Mixture:

Back 10

Composition and properties may vary.
Different amounts of sugar dissolved in water will
determine sweetness of water. Sugar water is an
example of a mixture.

Front 11

Chemical Compounds:

Back 11

Substance that can be broken
down into simpler substances. Water is a chemical
compound since it can be broken down into hydrogen and
oxygen by passing electric current through it.

Front 12

Element:

Back 12

Substance that can not be broken down
chemically into simpler substances. Hydrogen, oxygen,
nitrogen are example of elements.

Front 13

Reactants:

Back 13

One or more starting materials. Between
reactants, the “+” can be read as “reacts with”.

Front 14

products

Back 14

One or more substances formed as a result
of a chemical reaction. Between products, the “+” can be
read as “and”.

Front 15

fact

Back 15

113 Elements are known until today. Only 90 of these
elements occur naturally; the remaining are produced
artificially by chemists and physicist.

Front 16

The first letter is always capitalized and the second
letter is always a lower case.

Back 16

He (helium)

Front 17

fact

Back 17

All naturally occurring elements are not equally
abundant. Oxygen and silicon together constitute 75%
of the earth’s crust.

Front 18

chemical formula

Back 18

A notation for chemical compound
using element symbols and subscripts to show how
many atoms of each element are present.

Front 19

Metals:

Back 19

89 of the 113 elements are metals. They
appears on the left side of the Periodic Table.

Front 20

nonmetals

Back 20

Appear on the right side of the Periodic
Table. 17 elements are nonmetals.
Nonmetals are poor conductor of heat and electricity.

Front 21

Metalloids:

Back 21

Appear between metals on the left side
and nonmetals on the right side on the periodic table.
Their properties are between metals and nonmetals.

Front 22

Chemistry

Back 22

is the study of matter.

Front 23

Physical quantities

Back 23

Properties of matter such as height, volume, and
temperature that can be measured

Front 24

Weight is

Back 24

•a measure of gravitational pull on an
object.

Front 25

Mass is

Back 25

a measure of amount of matter in an
object.

Front 26

Two types of balances used for measuring mass in
the laboratory are shown below.

Back 26

a) Pan balance
(b) Electronic balance

Front 27

, the unit of density is

Back 27

grams per cubic centimeters (g/cm3).

Front 28

the unit of speed is

Back 28

meters per second (m/s)

Front 29

Meter (m) is

Back 29

the standard measure of length or
distance in both the SI and metric systems. One
meter is 39.37 inches.

Front 30

Volume is

Back 30

the amount of space occupied by an object

Front 31

The SI unit for volume

Back 31

is the cubic meter (m3).

Front 32

Volume is the amount of space occupied by an object.

Back 32

• 1L =0.001m3 = 1 dm3.

Front 33

fact

Back 33

Temperature is measured in Kelvin (K) in SI system and
in degrees Celsius (oC) in the metric system.

Front 34

fact

Back 34

Heat: kinetic energy of moving particles in a chemical
reaction.

Front 35

fact

Back 35

Temperature: a measure of how hot or cold an object is.

Front 36

fact

Back 36

Specific heat: amount of heat necessary to raise the
temperature of 1 g of the substance by 1oC.

Front 37

fact

Back 37

Specific gravity: density of a liquid divided by the density
of water.

Front 38

fact

Back 38

Density: relationship between mass and volume; grams
per milliliters for a liquid or gram per cubic centimeter for
a solid.

Front 39

fact

Back 39

Measurement of small or large numbers are usually
written in scientific notation, a product of a number
between 1 and 10 and a power of 10.

Front 40

fact

Back 40

• A measurement in one unit can be converted to
another unit by multiplying by a conversion factor.

Front 41

Energy: the capacity to supply heat or to do work.

Back 41

Potential energy – stored energy.
Kinetic energy – energy of moving particles.

Front 42

One Calorie is

Back 42

the amount of heat necessary to raise the
temperature of 1 g of water by 1oC.

Front 43

fact

Back 43

faTemperature in K = Temperature in oC + 273.15

Front 44

facts

Back 44

Zeroes at the beginning of a number are not
significant

Front 45

fact

Back 45

Zeroes at the end of a number and after the decimal
points are significant.

Front 46

1 kilogram (kg) 1000 grams

Back 46

0.001 kg
1000 mg
1 gram (g)

Front 47

1 microgram (μg) 0.001 mg

Back 47

0.001 g
1000 mg
1 milligram (mg)

Front 48

kilo hecto deka base

Back 48

deci centi milli micro nano

Front 49

mass---kg(si)

Back 49

g(metric)

Front 50

volume----cubic meter(cm3) si

Back 50

liter (metric)

Front 51

length is
time is

Back 51

meter
second

Front 52

temperqature- kelvin (si)

Back 52

celsius (metric)