Review Concepts

Front 1

Matter

Back 1

Any substance that has mass and occupies space

Front 2

Element

Back 2

The fundamental building blocks of matter, material that cannot be broken into simpler materials by ordinary chemical means

Front 3

H

Back 3

Hydrogen

Front 4

C

Back 4

Carbon

Front 5

N

Back 5

Nitrogen

Front 6

O

Back 6

Oxygen

Front 7

Na

Back 7

Sodium

Front 8

Mg

Back 8

Magnesium

Front 9

P

Back 9

Phosphorus

Front 10

S

Back 10

Sulfur

Front 11

K

Back 11

Potassium

Front 12

Ca

Back 12

Calcium

Front 13

Fe

Back 13

Iron

Front 14

Cu

Back 14

Copper

Front 15

I

Back 15

Iodine

Front 16

Atom

Back 16

The smallest indivisible piece of any element, smallest unit of matter that retains the chemical properties of the element

Front 17

Molecule

Back 17

Two or more atoms combined by chemical bond

Front 18

Compound

Back 18

A substance composed of molecules, two or more different elements

Front 19

Protons

Back 19

Mass = 1 amu

Charge = positive (+1)

Front 20

Neutrons

Back 20

Mass = 1 amu

Charge = neutron (0)

Front 21

Electrons

Back 21

Mass = 1/1800th amu

Charge = negative (-1)

Front 22

Nucleus

Back 22

Mass in center of atom, contains protons & neutrons, 99.9% of atom’s mass

Front 23

Electrons are found in the..

Back 23

Orbitals

Front 24

Orbital

Back 24

Pathways followed by electrons orbit the nucleus in pairs

Front 25

How many electrons in each orbital

Back 25

2 in the first

8 in each of the rest

Front 26

Orbitals energy

Back 26

Outer shells have more energy than inner shells

Front 27

Atomic #

Back 27

# of protons

Front 28

Atomic mass represents

Back 28

Theoretical mass of an atom, sum of the subatomic particles

Front 29

Atomic mass - atomic # =

Back 29

# of neutrons

Front 30

Isotope

Back 30

Atoms of the same element with different atomic mass

Front 31

Radioactive isotope

Back 31

Chemically unstable isotope, release particles and energy

Front 32

Octet rule

Back 32

8 electrons in each shell

Front 33

Outermost shell

Back 33

Valence shell

Front 34

Ion

Back 34

Atom w gained or lost electron to be more stable; full valence shell

Front 35

Cation

Back 35

Positive ions that form by losing electrons

Front 36

Anions

Back 36

Negative ions formed by gaining electrons

Front 37

Ionic Bond

Back 37

Atoms gain/lose electron to fill valence shell, opposite charged ions are attracted to each other

Front 38

Dissociation of an ionic bond

Back 38

Ionically bonded compounds dissociate into ions in charged environments

Front 39

Covalent Bond

Back 39

Atoms share electrons to fill their valence shell

Hint 39

Each atom contributes one electron to a shared pair

Front 40

Polar covalent bond

Back 40

Electrons not shared equally; one atom has higher electro negativity (much more massive)

Front 41

Hogs

Back 41

Shared electrons in a polar covalent bond

Front 42

Shared pairs travel

Back 42

Around both nuclei

Hint 42

Covalent bonds

Front 43

Polar

Back 43

Create charged regions on molecules, molecules w charged regions are polar

Front 44

Hydrophilic

Back 44

Water loving

Front 45

Hydrophobic

Back 45

Water fearing

Front 46

Water is polar

Back 46

Polar molecules are attracted to water

Front 47

Hydrogen bonds

Back 47

Weak bonds that form between polar molecules

Front 48

Van Der Waals forces

Back 48

Weak, random, electrical interactions between normally uncharged molecules

Hint 48

Due to random momentary variations in electron distribution

Front 49

Bases

Back 49

Substance that dissociates in water and combines w H+ ions

Front 50

Organic Molecules

Back 50

Molecules in living organisms or materials derived from living organisms; Hydrocarbons

Front 51

Tetravalent

Back 51

Forms four covalent bonds, can attach up to four different atoms together

Front 52

Isomers

Back 52

Different arrangements of a molecule