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Chemical Bonds
•Chemical bonds form when atoms are strongly attracted to one another
1) Ionic Bond2) Covalent Bond3) Metallic Bond
Compounds - Review•Compound: Substance that is composed of two or more
elements that are combined chemically •Properties of a compound are generally very different
from the elements that make it • Chemical Formulas:
• Formulas show the symbols on the ration of the elements in the compound
• Subscripts: tell the number of each element in the compound
Ex. C12H22O11
Review:
•Valence Electrons: Electrons in the highest energy level • The number of valence electrons largely determines the
chemical properties of an element. • To find the number of valence electrons, look at its group
number.
• Electron Dot Notation: represents the number of valence electrons
Ions - Review
• Ion: an atom or bonded group of atoms that has a positive or negative charge
• When atoms lose electrons and become positive ions, they always become smaller (compared to the neutral atom)• Loss of valence electron can leave an empty outer orbital resulting in a small
radius
• When atoms gain electrons and become negative ions, they become larger
Octet Rule
• Atoms tend to gain, lose (ionic bond) or share (covalent bond) electrons until they are surrounded by eight valence electrons
• An octet consists of 8 valence electrons
• Since the noble gases have eight electrons, we assume that an atom is stable when surrounded by 8 valence electrons
A gain of one electron gives chlorine an octet and converts a chlorine atom into a chloride ion. It has the same electron configuration as the noble gas argon.
Ionic Bond
• Type of chemical bond
• Electron transfers lead to forces holding atoms together
• Binds opposite charged ions together
• Formed by a METAL and a NONMETAL (or a group)
• Examples: NaCl (Sodium Chloride), Na2CO3 (Sodium Carbonate)
**To determine is an element is a metal, nonmetal or metalloid, look at its placement on the periodic table.
Ionic Bonding
• A bond forms when oppositely charged atoms are electrostatically attracted to one another as a result of the transfer of electrons
Classes of Ionic Bonds
1. Oxides • Compounds with ionic bonds between a metal and
oxygen• Example: MgO (Magnesium Oxide)
2. Salts • Generic name for most ionic compounds • Examples: NaCl (Sodium Chloride), ZnI2 (Zinc Iodide)
Intro to Ionic Names & Formulas
• Monatomic Ions: one-atom ions 1) Cation
• Positive ion formed by the loss of valence electrons
• Atom loses electrons to have an octet like the previous noble gases
• Naming: The cation name stays the same as the atom name • Example: Li Lithium
Li+ Lithium Ion
Monatomic Ions
2) Anion •A Negative ion formed by the gain of electrons •Atoms gain electrons to achieve an octet •Naming: For the anion, add the suffix –ide to the
root of the atom name• Example: Br bromine, Br - Bromide Ion
Oxidation Number (Oxidation State)
• The charge of a monatomic ion
• The number of electrons gained or lost to make an ion
• Monatomic Ion Trends: • Group 1: Plus 1 charge
• Group 2: Plus 2 charge
• Group 17: Negative 1 charge
• Group 16: Negative 2 charge
• Group 15: Negative 3 charge
Practice:
Write the symbol, name of the ion, and determine if it’s a cation or anion.
1. An iodine atom gains one electron
2. A strontium atom loses two electrons
3. A sulfur atom gains two electrons
4. An aluminum atom loses three electrons
Practice:
Atoms that tend to gain a noble gas configuration by LOSING valence electrons are
A. Metals
B. Nonmetals
C. Noble Gases
D. Representative Elements
Polyatomic Ions
• Polyatomic Ions:• Ions made up of more than one atom • Charge applies to the whole group • Never change the subscripts of atoms within the ion
• Example: CO32- (Carbonate)
• Oxyanion: • Ion with a nonmetal and one or more oxygen atoms
Polyatomic Ion Trends
NamingElement: S SulfurAnion: S2- Sulfide
SO52- Persulfate (+1 oxygen)
SO42- Sulfate
SO32- Sulfite (-1 oxygen)
SO22- Hyposulfite (-2 oxygen)
Ionic Bonds
• Ion Bond: Metal and Nonmetal Or
Positive Ion and Negative Ion
• When atoms transfer electrons, the atoms become bonded and form ionic compounds
• Although they are composed of charged ions, ionic compounds are electrically neutral (positive charge = negative charge).
Ionic Nomenclature
Writing Ionic Compound Formulas:
1. Write the cation and anion formulas with charges
2. Balance the charges with subscripts if necessary
3. Use parentheses around polyatomic ions that need a subscript added
4. Write the final neutral formula without charges
Practice:
•Potassium Permanganate: K+ MnO4
- KMnO4
•Aluminum Oxide:Al3+ O2-
add Al3+ Al3+ O2- O2- O2-Al2O3
•Copper (II) Hydroxide: Cu2+ OH-
add OH- Cu(OH)2
Naming Ionic Compounds
1. Cation name written first
2. Anion name written second
**Reminder: Use the roman numerals for most cations
More Practice:
•(NH4)2S
•AgC2H3O2
•CuCl
•LiHCO3
Ammonium Sulfide
Silver Acetate
Copper (I) Chloride
Lithium Bicarbonate
Properties of Ionic Compounds
• Crystal Lattice:
• Ions are arranged in a regular, repeating 3D pattern
• Each +ion is surrounded by – ions
• Overall the shape of the crystal depends on the relative number of + ions and – ions
Properties of Ionic Compounds
• Physical Properties:
• Particles are highly attracted to one another
• High melting & boiling points• Ionic crystals are hard, rigid, and
brittle• Can conduct electrical currents
• Electrolyte: an ionic compound whose aqueous solution conducts electricity• Aqueous Solutions: A substance
dissolved into water