Science Final

Front 1

suggested that the world was made of 2 things.
-empty space
-particles he called “atoms” (Greek word atoms, meaning indivisible)

Back 1

Democritus

Front 2

said everything was composed of 4 elements
1. air
2. fire
3. earth
4. water
He believed that matter was continuous and not made up of smaller particles.
He called this continuous substance hyle. Unfortunately this was accepted until the 17th century.

Back 2

Aristotle

Front 3

the smallest unit of matter that retains the properties of matter.

Back 3

atom

Front 4

region where the electrons are found

Back 4

electron cloud

Front 5

negative charge

Back 5

electron

Front 6

make up part of the nucleus and were found to have a positive charge

Back 6

protons

Front 7

make up the rest of the nucleus and have no charge. (not discovered until 1932)

Back 7

neutrons

Front 8

are similar to electrons but have no charge. They are produced in radioactive decay.

Back 8

neutrinos

Front 9

protons and neutrons are made up of particles called

Back 9

quarks

Front 10

proton quark

Back 10

( ^ ^ v )

Front 11

neutron quark

Back 11

( v v ^ )

Front 12

Atoms of the same element that have different atomic masses. This is due to their atoms having different numbers of neutrons.

Back 12

Isotopes

Front 13

Difference in an atom and a molecule

Back 13

Atoms are the smallest part of a substance that has all of the properties of the substance.
Molecules are two or more atoms chemically bonded together.

Front 14

Difference in a mixture and a compound

Back 14

Compounds are two or more different substances chemically bonded together. They have a definite composition and can only be separated by chemical means. Mixtures are a blend of substances. They are not chemically bonded and can be separated by physical means.

Front 15

Bonds that form as a result of atoms becoming ions and are drawn together by
their opposite charges (electromagnetic force).

Back 15

Ionic Bonding

Front 16

Characteristics of Ionic Bonding

Back 16

High melting points
Conduct electricity in a solution or molten form
Definite crystal shapes

Front 17

Examples of Ionic Bonding

Back 17

NaCl (sodium chloride)
CaCl2(calcium chloride)
NaOH (sodium hydroxide)
NH4OH (ammonium hydroxide)
CaCO3 (calcium carbonate)

Front 18

Bonds that form as a result of atoms sharing electrons to become more stable.

Back 18

Covalent Bonds

Front 19

Examples of Covalent Bonds

Back 19

H2O (water)
CO2 (carbon dioxide)
NH4 (ammonia)
CH4 (methane)
C6H12O6 (glucose)

Front 20

Characteristics of Covalent Bonds

Back 20

Low Melting point
Do not conduct electricity
Usually brittle solids

Front 21

Sodium

Back 21

is a metal and it loses electrons

Front 22

Chlorine

Back 22

is a nonmetal and gaines electrons

Front 23

Why is water a polar molecule?

Back 23

The bonds between the hydrogen atoms and the oxygen atom are covalent. The oxygen atom has a stronger pull on the pairs of electrons being shared. The electron
pairs are pulled toward the oxygen. This makes the oxygen side partially negative and the hydrogen side partially positive. This creates an intermolecular force between water molecules==drawing them together.

Front 24

Characteristics of water

Back 24

a) water is a liquid at normal temperatures (one of very few).
b) water does not evaporate quickly
c) water is polar.
d) ice floats in liquid water.
e) water is less dense as it approaches freezing (expands when it freezes).

Front 25

matter that has a definite shape and volume

Back 25

Solid

Front 26

matter that takes the shape of its container.

Back 26

Liquid

Front 27

matter that has no definite shape or volume.

Back 27

gas

Front 28

matter that is very hot, usually 5000°C or above.

Back 28

plasma

Front 29

only changes the appearance of the matter. It does not change the matter itself.

Back 29

physical change

Front 30

occurs when a chemical reaction takes place & something new is formed

Back 30

chemical change

Front 31

Changes of states of matter

Back 31

melting, boiling, condesation, sublimation

Front 32

process by which matter goes from a solid to a liquid

Back 32

melting

Front 33

matter changing from a liquid to a gas

Back 33

boiling

Front 34

matter changing from a gas to a liquid

Back 34

condensation

Front 35

matter changing directly from a solid to a gas. (dry ice, frozen CO2)

Back 35

sublimation

Front 36

Physical Properties:

Back 36

malleability
melting point
ductility
boiling point
conductivity

Front 37

Law of conservation of matter

Back 37

matter cannot be created nor destroyed

Front 38

Law of conservation of energy

Back 38

energy cannot be created nor destroyed. However, it can be changed
from one form to another.

Front 39

Law of conservation of matter and energy

Back 39

matter can be converted to energy & vice versus.

Front 40

transverse waves

Back 40

vibrations of molecules or particles of the medium are perpendicular to the direction of the wave.

Front 41

longitudinal waves

Back 41

vibrations are parallel to the direction of the wave

Front 42

wave medium

Back 42

air, water, rock, or steel

Front 43

an unbroken band of all colors

Back 43

continuous spectrum

Front 44

sources of continuous spectrum

Back 44

Hot, glowing metal (incandescent light bulb filament)
Molten metal (molten iron)
Hot compressed gases (plasma) deep inside stars

Front 45

a spectrum that consist of lines of color—not an unbroken band of colors.

Back 45

bright line spectrum

Front 46

sources of bright line spectrum

Back 46

hot glowing gas or vapor.
Examples--Hydrogen, Helium, Nitrogen, Mercury vapor, & Neon

Front 47

resembles a continuous spectrum with black lines.

Back 47

dark line spectrum

Front 48

Source of dark line spectrum

Back 48

Produced when a light source consisting of a continuous spectrum passes through a cool gas.
The cool gas will absorb the same colors it produces when it is hot.

Front 49

Aluminum

Back 49

Al

Front 50

Argon

Back 50

Ar

Front 51

Barium

Back 51

Ba

Front 52

Beryllium

Back 52

Be

Front 53

Boron

Back 53

B

Front 54

Bromine

Back 54

Br

Front 55

Cadmium

Back 55

Cd

Front 56

Calcium

Back 56

Ca

Front 57

Carbon

Back 57

C

Front 58

Chlorine

Back 58

Cl

Front 59

Chromium

Back 59

Cr

Front 60

Cobalt

Back 60

Co

Front 61

Copper

Back 61

Cu

Front 62

Fluorine

Back 62

F

Front 63

Gold

Back 63

Au

Front 64

Helium

Back 64

He

Front 65

Hydrogen

Back 65

H

Front 66

Iodine

Back 66

I

Front 67

Iron

Back 67

Fe

Front 68

Lead

Back 68

Pb

Front 69

Magnesium

Back 69

Mg

Front 70

Manganese

Back 70

Mn

Front 71

Mercury

Back 71

Hg

Front 72

Neon

Back 72

Ne

Front 73

Nickel

Back 73

Ni

Front 74

Nitrogen

Back 74

N

Front 75

Oxygen

Back 75

O

Front 76

Phosphorus

Back 76

P

Front 77

Potassium

Back 77

K

Front 78

Silicon

Back 78

Si

Front 79

Silver

Back 79

Ag

Front 80

Sodium

Back 80

Na

Front 81

Strontium

Back 81

Sr

Front 82

Sulfur

Back 82

S

Front 83

Tin

Back 83

Sn

Front 84

Zinc

Back 84

Zn