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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
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