IONIC BONDS

Ch 6.1

True False Statement True False

When an atom gains electrons it gets an (+) charge. When it loses

electrons it gets a (-) charge

Ionic bonds are between a metal and nonmetal

Anions are (-) and cations are (+)

Ionization energy is how much energy is needed to add an electron

Crystal lattice is a shape ionic compounds make

Electron Configuration

Stable- Highest occupied energy level is filled with

_______ Atom not likely to react

Electron Dot Diagram- Lewis Dot Shows Valance Electrons

Ionic Bonds

Transfer of electrons to become more stable

Na + Cl Na+ Cl-

Ion- atom with a positive or negative electric charge

Losing electrons + sign, Cation

Gaining electrons - sign, Anion

Transfer of Electrons Formation of Ions

Ionic Bonds Continued

Chemical Bond- force that holds atoms or ions together

Ionic Bond- force that holds cations and anions together

- the amount of energy used to remove an electron

Lower I-energy = easier to remove

Formation of Ionic Bonds Ionization Energy

Ionic Compounds

Compounds that contain ionic bonds

Usually a metal bonded to a nonmetal

Chemical Formulas- notation that shows what elements a compound contains and the ratio of atoms or ions of those elements

Crystal Lattice

Attraction between elements, that keeps the ions in fixed positions

Rigid, framework= lattice Solids with lattice structures are called

crystals

Ionic Properties

Strong attractions between ions within a crystal lattice

When melted, great conductors of electricity

Shatter when struck= _______

COVALENT BONDS

Ch. 6.2

True False Statement True False

Covalent bonds are between 2 nonmetals, that share valence

electrons

Bonds can be single, up to quadruple

Polar covalent bonds, are not shared equally

Nonpolar bonds are stronger than polar bonds

Polar bonds include, (-) and (+) signs to show polarity

Covalent Bonds

Chemical bond where 2 atoms share a pair of valence electrons

Molecule- neutral group of atoms, joined by covalent bonds

Attraction between shared electrons and protons hold atoms together

Sharing Electrons Molecules of Elements

Covalent Bonds

Multiple Bonds Single Bonds

H-H Double Bonds

C=C Triple Bonds

N N

Usually a nonmetal bonded with a nonmetal

Unequal Sharing

Polar Covalent Bonds Electrons are not

shared equally Atom with greater

attraction for electrons has partial – charge

Atom with less attraction has partial + charge

Nonpolar Covalent Bonds Equal sharing

Attraction Between Molecules Polar bonds are stronger than nonpolar

bonds

NAMING COMPOUNDS & WRITING FORMULAS

Ch. 6.3

True False Statement True False

When naming ionic compounds, anions are written 1st, followed by

cations

When naming covalent compounds, you must use a prefix for every

element

Polyatomic ions are covalently bonded atoms with a (-) or (+)

charge

Oxidation #s tell the charge the ion would have if it gained or lost

electrons

-ide ending is added to the 1st elements name in the compound

Naming Ionic Compounds

Metal to nonmetal 1st- Cation

Metal without change

Sodium 2nd- Anion

Nonmetal with suffix –ide

Chlorine = chloride 3rd- Combine

Sodium chloride

Examples: LiF

KO

CuS

BeCl

Formulas for Ionic CompoundsCalcium chloride 1st- Write Symbols

Ca Cl

2nd- Locate Ca ClCation anion

3rd- Find oxidation # Ca+2 Cl-1

Lose 2 electrons Gain 1 electron

4th- Criss cross, then write as subscript CaCl2

Transition Metals

Get oxidation # from anion Must be neutral

Backward crisscross

Iron(II) oxide Fe?O-2

Fe+2O-2

FeO

Naming Examples

CoBr2

Cobalt(II) bromide CrCl3

Chromium(III) chloride MnO2

Manganese(IV) oxide AgO

Silver(II) oxide

Formula Examples

Iron(II) oxide FeO

Iron(III) oxide Fe2O3

Gold(II) oxide AuO

Platinum(III) oxide Pt2O3

Polyatomic Ions

Covalently bonded group of atoms with either a positive or negative charge

Most common list pg 173

Math Practice pg 174

1.

2.

3.

4.

Naming Molecular Compounds 2 Nonmetals 1st- Count how

many of each element Use prefixes Di-, pent-

2nd- Add element name and ending Dinitrogen

pentoxide

Naming Examples

CO Carbon monoxide

CO2

Carbon dioxide N2O4

Dinitrogen tetraoxide N2O

Dinitrogen monoxide

Formula Examples

Dicarbon tetraoxide C2O4

Tetraboron dichloride B4Cl2

Arsenic hexoxide AsO6

Silicon pentsulfide SiS5

STRUCTURE OF METAL S

Ch. 6.4

True False Statement True False

Metallic bonds are between a metal and a transition metal

Metal bonds have a crystal lattice structure

Alloys are mixtures, in which 1 is a metal

Alloys are homogenous mixtures

Alloys can be designed with specific properties for different tasks

Metallic Bonds

Attraction between a metal cation and the shared electrons surrounding it

2 metals, with no nonmetal to accept electrons

Cations form a lattice=strong bonds between cations and valence electrons Neutral charge

Properties of Metal

Mobility of electrons

Conduct electric current Shared electons

Malleable & Ductile Flexible lattice

Alloys

Mixture 2 or more elements 1 is a metal heterogenous

Characteristics of metals

Alloys

Bronze Tin Brass Harder, stronger

than each metal alone

Iron Carbon Chromium Different mixtures

for different needs

Copper Steel