Chapter 2

Front 1

Matter

Back 1

Anything that occupies space and has mass

Front 2

Mass

Back 2

Amount of space an object takes up

is dependent on density

not dependent on gravity

Front 3

Weight

Back 3

measurement of gravitational pull on an object

how much gravity is pulling down

Front 4

Element

Back 4

matter that cannot be decomposed

made up of one atom

Front 5

Atom

Back 5

2 regions:

nuclear

electron shell or cloud

Made up of subatomic particles

protons+

neutrons0

electrons-

Front 6

Atomic Symbol

Back 6

official abbreviation of an element

Front 7

Atomic Number

Back 7

the number of protons in an atom

Front 8

Atomic Mass Number
(mass number)

Back 8

the number of protons+neutrons

Front 9

Neutron Number

Back 9

atomic mass number minus atomic number

Front 10

Electron number

Back 10

in a normal atom (electrically neutral) the number of protons=number of electrons

Front 11

Electron Placement

Back 11

Electrons travel around the nucleus in shells (energy levels)

Front 12

1st Shell

Back 12

holds up to 2 electrons

Front 13

2nd Shell

Back 13

holds up to 8 electrons

Front 14

3rd Shell

Back 14

holds up to 8 electrons

Front 15

4th Shell

Back 15

holds up to 8 electrons

Front 16

Deuterium

Back 16

Used to make heavy water

Front 17

Ion

Back 17

and electrically charged atom

atoms are most stable when they have a full outer shell
2 types of ions:

Cations

Anions

Front 18

Cations

Back 18

a positively charged atom
Na+

Front 19

Anion

Back 19

A negatively charged atom

Cl-

Front 20

Isotopes

Back 20

Atoms with the same atomic number, but with different atomic masses because of varying numbers of neutrons

Front 21

Chemical Bonding

Back 21

How atoms stick together

3 categories:

Ionic bonds

Covalent bonds

Hydrogen bonds

Front 22

Ionic Bonds

Back 22

Occurs between cations and anions

e- donors (cations) and e- acceptors (anions)

metals and non-metals

e- are transferred, not shared

forms compounds

Front 23

Covalent Bonds

Back 23

electrons are shared

forms molecules

uses covalent bonding to stick them together

occur between non-metals

2 kinds of covalent bonds:

non-polar

polar

Front 24

Non-polar Covalent Bonds

Back 24

sharing of e- is equal

hydrophobic (won't dissolve in water)

Front 25

Polar Covalent Bonds

Back 25

sharing of e- is unequal

hydophilic (like water)

because of unequal sharing of e-, the molecule has a slight charge at its ends

Front 26

Hydrogen Bonds

Back 26

weak electrostatic bond that occurs between polar molecules

also known as intermolecular bond

occurs between 2 different molecules

proteins- aids protein structure

DNA-holds two strands of DNA together

gives water its special properties

Front 27

Special Properties of Water

Back 27

temperature stable

solvent properties

cohesive and adhesive properties

Front 28

Water is Temperature Stable

Back 28

takes a lot of energy to change the temperature

Front 29

Water has Solvent Properties

Back 29

water is really good at dissolving things

because of polar covalent bonds

universal solvent

dissolves polar substance and ionic

Front 30

Water has Cohesive and Adhesive Properties

Back 30

water molecules stick together

gives the meniscus when measuring water

surface tension

Front 31

Acid

Back 31

any substance that donates hydrogen ions (H+)
HCl--H+ + Cl

Front 32

Base

Back 32

any substance that accepts hydrogen ions (h+)

Alkaline=basic

common base is hydroxide OH-

H+ + OH= H2O

Front 33

pH Scale

Back 33

Measues concentration of [H+]
Scale of 0 to 14 is used

Front 34

pH=7

Back 34

pure water

Front 35

pH<7

Back 35

lower pH=stronger acid

Front 36

pH>7

Back 36

higher pH=stronger base

Front 37

Buffers

Back 37

any substance that can soak up or release H+

helps to prevent wide swings in pH

Front 38

Salts

Back 38

substance made by combining strong acids and strong bases