Chemistry - Ch. 5, 12

Front 1

Electron charge:

Back 1

-1

Front 2

Proton charge:

Back 2

+1

Front 3

Neutron charge:

Back 3

0 (no charge)

Front 4

Electron atomic mass unit:

Back 4

0 (no mass)

Front 5

Proton atomic mass unit:

Back 5

1

Front 6

Neutron atomic mass unit:

Back 6

1

Front 7

Neutrons=:

Back 7

ATOMIC MASS (-) MINUS ATOMIC NUMBER (# OF PROTONS)

Front 8

Protons and neutrons located:_______
electrons located:________

Back 8

Inside the nucleus; outside the nucleus

Front 9

Chemical bonding:

Back 9

Attractive forces that hold atoms together

Front 10

The driving force that causes chemical reactions to occur:

Back 10

Minimization of energy

Front 11

Valence electrons:

Back 11

Electrons in the outermost shell of an element

Front 12

Noble gases have:

Back 12

An octet of 8 valance electrons

Front 13

IONS:

Back 13

When an atom gains or loses electrons

Front 14

Ionic bonds usually happen between:

Back 14

metal and non-metal elements

Front 15

Writing an element as an ion:

Back 15

Element+ charge requirement
e.g. Ca 2+
+= number of electrons they want to give up; --- = number of electrons they want to receive)

Front 16

Ionic bonds have a:

Back 16

High melting point

Front 17

Solutions that conduct electrical currents because of the movement of ions are:

Back 17

Electrolytes

Front 18

Covalent bond:

Back 18

When atoms are sharing electrons

Front 19

Covalent bonds are still trying to achieve:

Back 19

Octet (8 electrons in outermost shell)

Front 20

The term molecule only applies to:

Back 20

Covalent bonds

Front 21

Polarity exist when there is:

Back 21

Unequal sharing of electrons (electronegativity) in a covalent bond (oxygen for example H - - O - - H, oxygen has partial negative, hydrogen has partial positive)

Front 22

Noble gases have no:

Back 22

Electronegativity

Front 23

If there is no difference in electronegativity, there will be no:

Back 23

polarity

Front 24

A bond in which one pair of electrons is shared between two bonded atoms:

Back 24

A single bond

Front 25

A bond in which two pairs of electrons are shared between the two bonded atoms:

Back 25

A double bond

Front 26

A bond in which three pairs of electrons are shared between the two bonded atoms:

Back 26

A triple bond

Front 27

Identifying an ion is when there is a difference between:

Back 27

Protons and Electrons

Front 28

written isotopes: top number =

Back 28

# of protons + # of neutrons (atomic mass)

Front 29

written isotopes: bottom number =

Back 29

# of protons (atomic number)

Front 30

the written form of isotopes is called:

Back 30

nuclear symbol
eg: 12 C
6

Front 31

the nuclear atom was concieved by:

Back 31

Rutherford

Front 32

isotopes are defined as:

Back 32

atoms of the same element that have different masses

Front 33

polarity is dicated by:

Back 33

electronegativity (usually increases moving to the right of the periods)

Front 34

Two or more atoms of the same elements that have different atomic masses because of different numbers of neutrons:

Back 34

Isotopes

Front 35

A sample consisting of only one kind of matter, either compound or element:

Back 35

A pure substance

Front 36

A reaction that gives off energy to its surroundings:

Back 36

Exothermic reaction

Front 37

A change that absorbs energy from the surroundings:

Back 37

Endothermic reaction

Front 38

Pertaining to a bond or molecule having an asymmetrical distribution of electric charge:

Back 38

Polar bond

Front 39

The formula as of the beginning substances that are written to the left of an arrow:

Back 39

Reactants