Honors Chemistry Review Topics

CHAPTER 7– “Periodic Properties of the Elements”

Development of the Periodic Table – Mendeleyev and Mosley

Effective Nuclear Charge

Sizes of Atoms and Ions

Periodic trends in Atomic Radii of atoms and ions

Ionization energy

Values of successive ionization energies I₁, I₂, I₃ etc. and their relationship to electron configuration

Periodic trends in first ionization energies

Electron configuration of ions

Electron affinities

Properties of metals:

            Shiny, mostly silvery, solids (except Hg), malleable and ductile, good conductions

            Low ionization energies so form + ions

            Compounds of metals with nonmetals tend to be ionic

            Metal oxides (base anhydrides)– react with water to form bases or react with acids to form salts and water

Properties of nonmetals:

            Vary greatly in appearance, brittle, poor or non conductors

            Have high electron affinities so form “– “ ions when they react with metals

            Compounds containing only nonmetals are molecular (covalent) substances

Nonmetal oxides (acid anhydrides) – react with water to form acids (acid rain); or react with bases to form salt and water

Metalloids have properties between metals and nonmetals

Group IA – Alkali metals - exist in nature only as compounds, lowest I₁, react with nonmetals to form salts, react with water to form base and H₂

Group IIA – Alkaline earth metals – similar to Group IA, but react slower

Metal reactivity increases as you go down in a family – lower ionization energy

Nonmetal reactivity decrease as you go down in a family – lower electron affinity

Group VIA – Oxygen family

            Oxygen is O₂, ozone is O₃. (allotropes)

Group VIIA – Hallogens (X) –React with metals to form salts

Group 8A – Noble Gases – filled s and p orbitals so are non-reactive except in extreme conditions

Chapter 8 – “Basic Concepts of Chemical Bonding”

Types of chemical bonds:  ionic, covalent, metallic

Lewis dot symbols

Octet rule – full s and p orbitals

IONIC BONDING:

Electrons are transferred from one atom to another

Isoelectronic – atoms and ions with the same electron configuration

Lattice energy – energy required to separate one mole of ionic solid into its gaseous ions –Increases as ion charges increase and as radii decrease

Born-Haber Cycle – calculation of lattice energy

Electron configuration of: 

a) Representative elements (Groups 1A-8A) full s and p orbitals

b) Transition Metal ions – use valence s orbital, then previous d orbital if needed

c)  Polyatomic ions – covalently bonded group with an overall charge

COVALENT BONDING:

Most compounds are covalent

Represented by Lewis Dots shared between atoms

# of electron pairs:  HONC (1,2,3,4 pairs)

Distance between bonded atoms decreases as # of bonds increases

Bond Polarity:  degree of sharing of electron pairs:

            Equally shared = non-polar covalent bond e.g. H₂

            Not equally shared = polar covalent bond e.g. HCl

Shapes:  VSEPR determines shapes: 

            Linear, angular (or planar or bent), tetrahedral (3-D)

Shapes determine molecular polarity

Electronegativity:  ability of an atom in a molecule to attract electrons: if difference is high = ionic bond; If medium = polar covalent bond; low or zero = non-polar covalent bond

Resonance structures