1. Be able to tell the difference between observation and conclusion.
  1. Atlantic Pacific rule. (If the number has a decimal (Pacific), start counting from the left side starting with the first nonzero digit. If there is no decimal (Atlantic), start counting from the right side starting with the first nonzero digit)
  1. When doing calculations, the answer can only have as many significant figures as the least one in the calculation. (22.3 x 8.6785 = 193.53055 or194?)
  1. Know how to convert between prefixes. ( Use the number line)

K, h, da * d , c, m

  1. Know how to calculate percent error.

(Experimental value) − (true value)
% error= ――――――――――――― × 100
true value

  1. Characteristics of a solid, liquid and gas.
  1. Define sublimation, condensation, melting, boiling.
  1. Know the meaning of (s), (l), (g) in a chemical equation. How is phase transformation indicated? H20(l) ----- H20(g).
  1. Know the difference between a chemical and physical property?
  1. Know how to calculate density? density = mass/volume
  1. Know the charge and mass of a proton, neutron, and electron?
  1. Know what Rutherford’s experiment concluded? (Ernest Rutherford publishes his atomic theory describing the atom as having a central positive nucleus surrounded by negative orbiting electrons. This model suggested that most of the mass of the atom was contained in the small nucleus, and that the rest of the atom was mostly empty space.)
  1. When electrons move up or down in atomic energy levels, what happens to the energy (Given off or absorbed)?
  1. Know how to calculate average atomic mass given mass of isotopes?

Average Atomic Mass = % as decimal x mass + % as decimal x mass + % as decimal x mass.

  1. How can you tell you have an isotope, given the symbol? Pu-244, Pu-243
  1. Know how to determine protons, neutrons, and electrons, from the periodic table, or chemical symbol (both)

24

Mg or Mg-24 *number is atomic mass (weight) and = P+N

12

Top number is Atomic mass (weight) and equals protons ‘+’ neutrons

Bottom number is Atomic number and equals protons.

Protons will equal the number of electrons in a neutral atom.

  1. Know how to determine protons, neutrons, and electrons, from the periodic table, or chemical symbol (both) for ions. Same as #16 except for the following:

If you have a ‘-‘add electrons for each negative charge (-2 would be add 2 electrons, ‘-‘add 1 electron.

If you have a ‘+’ subtract 1 electron or each ‘+’ charge. (+3= subtract 3 electrons, ‘+’ = subtract 1 electron

  1. Flame test colored light is given off when electrons emit or absorb energy when moving from higher to lower energy levels? Energy is absorbed when electrons move to higher energy levels and given off when electrons move to lower energy levels.
  1. Periodic trend for ionic radius and atomic radius?

See handout

  1. Chemical characteristics are determined by what? Elements in the same group have similar chemical characteristics due to what? (valence electrons)
  1. When an ionic bond forms what happens to the size of the metal and nonmetal atoms? (In ionic bonding, electrons are completely transferred from one atom to another. Atoms that gain electrons (Nonmetals) become bigger, while atoms that loose electrons (metals) become smaller. Metals form ‘+’ ions bygiving up electrons to nonmetals, which form ‘–‘ions.
  1. How can you tell which element has the greater ability to attract electrons, given the periodic table?Electro negativity number. Increases as you go up and to the right on the Periodic Table.
  1. Ionic and covalent bonds share or exchange electrons?
  1. Why do metals conduct electricity?
  1. Ionization energy? How can you tell which atom has the lowest or highest?

See Periodic trend handout. (Increases as you go up and to the right on the Periodic Table.)

  1. Periodic trend for electro negativity?

See Periodic trend handout. (Increases as you go up and to the right on the Periodic Table.)

  1. Where are metals and nonmetals located on the periodic table?
  1. Why is the atomic radius of a metal atom greater than that of its ion?

Metal looses an electron to form “+” ion and gets smaller as a result.

  1. What happens during boiling of water? Do chemical bonds break or intermolecular forces?
  1. Electro negativity and bond types?
Bond type by Electro negativity

Electro negativity Bond

Difference type

< 0.4 Nonpolar covalent

0.5 to 1.9 polar covalent

>2.0 ionic

  1. When drawing a Lewis structure how do you determine the central atom?

Atom with the highest electro negativity.

  1. Given a Lewis dot diagram, determine the correct electron configuration? (only the last energy level)
  1. Chemical bonds form so as to gain 8 electrons in its highest energy level. (Valence) octet rule.
  1. How can you tell the valence electrons given the electron configuration? The exponents above the letters after the highest energy level(number)
  1. Lewis structures and single, double, triple covalent bonds?
  1. How is an electrolytic solution formed? (metals dissolved in water)
  1. What is lattice energy? (ionic bond energy needed to break bond)
  1. Compare ionic and covalent bonds in strength, melting points, conduction, and solubility?
  1. Electrons in the electron sea model of metallic bonding?
  1. Molecular shape?

Bond angle Dimension

1. Linear- 180 2D

2. Trigonal planar 120 2D

3. Tetrahedral 109.5 3D

4. Pyramidal 107 3D

5. Bent 105 3D

  1. What is a polar bond, what is a polar molecule?

. Determining Polarity

  1. A polar molecule is called a dipole and has one end with a positive charge and one end with a negative charge.
  2. A molecule’s polarity is determined by its shape and the polarity of its bonds.
  3. A molecule that contains only nonpolar bonds is always nonpolar.
  4. A molecule with polar bonds may be either polar or nonpolar.
Bond type by Electro negativity

Electro negativity Bond

Difference type

< 0.4 Nonpolar covalent

0.5 to 1.9 polar covalent

>2.0 ionic

  1. Ionic formula (words to formula) criss-cross ion charge
  1. Naming ionic compounds? (Formula to words) (roman numerals)
  1. Naming covalent compounds (formula to words)?

The following prefixes are used.

mono-1 di-2

tri-3tetra-4

penta-5hexa-6

hepta-7octa-8

nona-9deca-10

  1. Naming acids? See Table
  1. When balancing chemical equations, do you adjust coefficients or subscripts? Always coefficients.
  1. Conservation of mass for chemical reactions (products – reactants) Will be equal
  1. Balance a chemical equation? Left to right, add or change coefficients only.
  1. Types of reactions? (Synthesis, decomposition, single replacement, double replacement, combustion).

A + B yield AB Synthesis

AB yields A + B Decomposition

A + BC yields AC + B Single replacement

AB + CD yields AC + BD Double Replacement

Oxygen on the left yields water on the right = Combustion

Short cuts:

No ‘+’ on left = decomposition

No ‘+’ on the right = synthesis

Single element on left + Compound = single replacement

Two compounds on left = double replacement

Oxygen on left with water on right = combustion

  1. Net ionic equations?
  1. How to go from molecular to empirical formulas and back? Reduce subscripts to smallest number divisible by all subscripts. Empirical to molecular = multiple subscripts by 2.