Physical Science Chapter 6

Front 1

Chemically Stable

Back 1

If an atoms outer energy level is completely filled with electrons.

Front 2

Dot Diagrams

Back 2

The symbol for an atom which has the valence electrons represented by dots.

Front 3

Superscript

Back 3

is written above

example: O^2-

Front 4

Subscript

Back 4

is written below

example: O2

Front 5

Ions

Back 5

Atoms that are either positively or negatively charged, because of the gained or lost valence electrons.

Front 6

Anion

Back 6

ions with a negative charge.

(Nonmetals) N3- O2- Cl1-

to name an anion, you change the ending to “ide” (example: nitride ion, oxide ion, chlorideion)

Front 7

Cation

Back 7

ions with a positive charge.

(Metals) K1+ Ca2+ Al3+

to name a cation, you change nothing

(example: potassium ion or calcium ion)

Front 8

Chemical bond

Back 8

A force that holds together the atoms or ions together as a unit.

Gaining, losing, and sharing electrons are how atoms form chemical bonds, and by doing so, they become more stable.

Front 9

Ionic Bond

Back 9

The force that holds cations and anions together to form an ionic compound.

Front 10

Chemical Formula

Back 10

Tells what elements a compound contains and the ratio of the atoms of those elements.

Front 11

Electronegativity

Back 11

How strongly an atom attracts electrons in a bond.

It increases as you go to the right on the periodic table, and increases as you go up.

Front 12

Molecules

Back 12

Neutral particles formed because of valence electron sharing.

Front 13

Covalent Bond

Back 13

A bond that forms between atoms when they share valence electrons. Ex: HCl, H2O, N2

Front 14

Diatomic Molecules

Back 14

Two atoms of the same element joined together by covalent bonds.

Front 15

Polar Covalent Molecule

Back 15

One that has a positive end and a negative end.

Front 16

Nonpolar Covalent Molecule

Back 16

One that does not have oppositely charged ends.

Front 17

Oxidation Number

Back 17

A positive or negative number assigned to an element to show its combining ability in a compound - the oxidation number indicates how many electrons an atom has gained, lost, or shared when bonding with other atoms/body.

Front 18

Binary Compound

Back 18

A compound that is composed of only two elements.

Front 19

Polyatomic Ion

Back 19

A positively or negatively charged group of atoms.

Front 20

Metallic bond

Back 20

The attraction between a metal cation and the shared electrons around it.

Front 21

Alloy

Back 21

A mixture of two or more elements, at least one of which is a metal.

Front 22

Bronze

Back 22

An alloy of copper and tin.

Front 23

Brass

Back 23

An alloy of copper and zinc.

Front 24

Steel

Back 24

An alloy of iron and carbon.