Ionic Bonding and Naming

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Elements vs. Compounds• An element cannot be ___________ down or _____________ into

simpler substances by chemical means.

• Elements are the _________ forms of matter that can exists in normal laboratory conditions.

Examples: _______, Helium, __________

• A compound is made up of ____ or ________ different elements ______________ bonded together.

• Compounds can only be broken down into simpler substances by ____________ ____________.

Examples: _______, Sand, _______________

broken changed

simplest

MercuryGold

2 morechemically

chemical reactions

Water NaCl (table salt)

Mixtures• Mixtures are a physical blend of two or more substances mixed

together.” The parts can be separated by _____________ means or ____________ changes.

There are 2 types of mixtures:

(1) _________________ Mixtures: the parts mixed together can still be distinguished from one another...NOT uniform in

composition.

Examples: chicken soup, fruit salad, _____, sand in water

(2) _________________ Mixtures: the parts mixed together cannot be distinguished from one another...completely uniform in

composition.

Examples: ______, Kool-aid, ________, salt water, milk

• Another term for a homogeneous mixture is a “______________.”

physicalphysical

Heterogeneous

Homogeneous

dirt

Air Brass

solution

Heterogeneous Mixtures

Homogeneous Mixtures

Classification of Matter

Ionic Bonding & Ionic CompoundsIonic Bonds

• Form when ___________ transfer their _____________ electrons to a _______________.

• The forces of attraction between the ____________ (+) and the _____________ (-) bind the compound together.

How to Represent an Ionic Bond

(1) Electron Configuration:

Na 1s2 2s2 2p6 3s1

Cl 1s2 2s2 2p6 3s2 3p5

metals valencenonmetal

cationanion

Na… ___ 3s

↑

Cl… ___ ___ ___ ___ 3s 3p

↓↑ ↑ ↑↓ ↓ ↓

How to Represent an Ionic Bond

2) Bohr Model

Lithium Fluorine

Practice Problems:

3) a) Draw the electron dot notation for a sodium atom.

b) Draw the electron dot notation for a sodium ion.

(4) a) Draw the electron dot notation for a oxygen atom.

b) Draw the electron dot notation for a oxygen ion.

Na

[Na+1]

O

[ O -2]

How to Represent an Ionic Bond

3) Electron Dot Notations:

Na + Cl [ ] [ ]

Practice Problems: (1) Draw the electron dot notation for the formation of an ionic compound between calcium and oxygen.

(2) Draw the electron configuration notation for the formation of an ionic compound between magnesium and fluorine.

Na+1 Cl -1

Properties of Ionic Compounds and Covalent Molecules

Ionic:

•_______________ of electricity when dissolved water or melted.

•formed between __________ and _________________

•have _________ melting points

•usually ________ soluble in water

• form ___________________ solids

Conductors

metals nonmetals

high

very

ionic crystalline

(dissolved salt)

Crystalline Patterns

Pyrite

• mineral form of the iron (IV) sulfide (FeS2) with a gold-like appearance, making it also known as "fool's gold"

Gypsum

• Gypsum is a very soft mineral composed of calcium sulfate dihydrate, with the chemical formula CaSO4·2H2O.

Demonstration

good conductor

poor conductor

nonconductor

PureH2O

great conductor

Ionic Names & Formulas

• Ionic Compounds (“________”):

–Name or formula starts with a _________ (or NH4 +,

ammonium).

–Other quick ways to tell if the compound is ionic:

• formula uses parentheses

Example: ________________

• formula contains more than 2 elements (capital letters)

Example: ________________

• name uses Roman numerals

Example: ________________

• name ends in “-ate” or “ite”.

Example: _________________

salts

metal

Ca(OH)2

FeCrO4

lead(II) chloride

barium sulfate

Writing Formulas for Ionic Compounds

• Step 1-- Use your ion sheet and find the ions and their charges.

• Step 2-- “Cross the charges” if they don’t balance out.

• Step 3-- Use parentheses around polyatomic ion “chunks”.

Practice Problems: Write the formula for each ionic compound.

copper(II) bromide ____________________

aluminum nitrite _________________________

barium hydrogen carbonate ___________________________

Cu+2Br -1 = CuBr2…(don’t show 1’s)

Al+3 NO2 -1 = Al(NO2)3

Ba+

2

HCO3-1 = Ba(HCO3)2

AcidsWhat makes something an acid?

Acid Properties:

(1) tastes _______-- _______________

(2) corrosive to _________

(3) contains [ ___ ] (or [ _____ ] = “_______________” ions)

(4) proton ([ ___ ]) __________-- Brønsted-Lowry Theory

Example: HCl + H2O ______ + ______

sour lemons

metals

H+ H3O+ hydronium

H+ donor

Cl− H3O+

Examples of Common Acids:

• Pepsi, _________ juices, ___________, stomach acid, battery acid, _____________, ______

citrus aspirinvinegar DNA

Acids

• All acids begin with the element ________________.

• General format: H(X), where “(X)” represents the ______________.

• There are 2 general types of acids:

– If the name of “(X)” ends in –ite or –ate, then it is an _________ acid.

– If the name of “(X)” ends in –ide, then it is a ____________ acid. The acids

just contains ____ elements, hydrogen and a nonmetal. (There’s NO oxygen!)

hydrogen

anion

oxy-

binary2

Naming Oxy-Acids

1. If the name of “(X)” ends in –ate… (anion root)-ic acid

2. If the name of “(X) ends in –ite… (anion root)-ous acid

Practice Problems: Name these acids.

H2SO4 H3PO3 HNO3 H2CO3 HC2H3O2

HClO2

Naming Binary Acids

If the name of “(X)” ends in –ide… hydro- (anion root)-ic acid

Practice Problems: Name these acids.

H2S HCl HF

sulfuric acid

phosphorous acid

nitric acid

carbonic acid

acetic acid

chlorous acid

hydrosulfuric acid hydrochloric acid hydrofluoric acid

Writing the Formulas for Acids

FIRST You must determine the formula for the anion, “(X)”.

1. If the acid’s name starts with “________” (and ends in “–ic”), the name of the anion used ends in “_______”. Therefore, it is a _________ acid. (There’s only hydrogen and one other nonmetal in the formula!)

• The subscript on the hydrogen equals the anion’s charge!

Examples: hydrobromic acid = ________

hydroiodic acid = _______

hydrosulfuric acid = ________

hydro-ide

binary

HBr

HI

H2S

2. If the acid’s name ends with “______” without the “hydro-” prefix, the name of the anion used ends in “_______”. Therefore, it is an ____ acid.

• The subscript on the hydrogen equals the anion’s charge!

Examples: perchloric acid = __________

oxalic acid = ___________

3. If the acid’s name ends with “______”, the name of the anion used ends in “_______”. (It’s is also an oxy-acid.)

• The subscript on the hydrogen equals the anion’s charge!

Examples: hypochlorous acid = __________

nitrous acid = ____________

sulfurous acid = ____________

-ic-ate

oxy-

HClO4

H2C2O4

-ous-ite

HClO

HNO2

H2SO3