"Advanced Chemistry 10 - Summary of Semester #1"

The agreement of a particular value with the true value.

The degree of agreement among several measurements made in the same manner.

Two properties that are dividing one by the other and gives a constant value.

-Straight Line

Two quantities where their product is constant.

-Curve Line

Le Systeme International d’Unites

Combinations of SI base units

Numerical information

Non-numerical information

Move decimal point so the number fits between 1 and 10.

record all digits.

read all certain digits and one uncertain digit.

All the digits known with certainty plus one final digit, which is somewhat uncertain or estimated.

Decimal absent (right).

Decimal present (left).

use the fewest number of decimal places.

use the least amount of significant digits.

Skill used to convert units using conversion factors and proving the units.

Mass/Volume

-directly proportional

Discovered the electron (cathode ray tube)

Measured the charge of the electron (oil-drop experiement).

Gold foil experiement - found details of the atom’s structure - (nucleus was positively charged, atom is mostly space).

Proposed a model in which electrons surrouned the positively charged nucleus as the planets surround the sun (planetary model).

Explained the number of particles in a mole (found a relationship between mass and the number of atoms).

Mass is neither created nor destroyed.

A given chemical compound always contain its component elements in fixed ration (by weight) and does not depend on its source and method of preparation.

When two elements combine to form one compound, the mass of one element, when combined with a fixed mass of the other element, will always be ratios of whole numbers.

1. All matter is composed of extremely small particles called atoms.

2. Atoms of a given element are identical in size, mass, and other properties; atoms of different elements differ in size, mass, and other properties (not true).

3. Atoms cannot be subdivided, created, or destroyed (not true).

4. Atoms of different elements combine in simple whole number ratios to form chemical compounds.

5. In chemical reactions, atoms are combined, separated, and rearranged.

Center of the atom

Positive charge

Neutral charge

Negative charge

Number of protons. Shown on the periodic table.

Protons + Neutrons

Atoms that have the same number of protons and a different number of neutrons.

Mass of one mole of a pure substance. Units are g/mol. Round to 2 decimal places.

6.022x10^23

particles and waves.

Distance between two consecutive corresponding points on a wave.

Directly proportional

Number of complete waves that pass a point in 1 second.

Lowest energy state.

Highest energy state.

electrons.

It is impossible to determine simultaneously both the position and velocity of an electron or any other particle.

The quantum theroy.

Combined mathematical equations and conluded that ANYTHING with mass and velocity has a corresponding wavelength.

Specify the properties of an atomic orbital and the properties of electrons in an orbital.

Electrons enter the lowest energy level possible

No two electrons can have the same set of quantum numbers and therefore will have opposite spins.

One electron enters an orbital of equal energy parallel in spin before pairing begins.

8 electrons in the “s” and “p” sublevels.

Particles of light. Discovered by Einstein.

A huge, often sudden, increase or advance.

releases the excess energy.

Describes the size of orbital.

Describes the shape of the sublevel.

Describes the orientation about the azes.

Describes the rotation of an electron.

Responsible for arranging the periodic table by increasing ATOMIC MASS.

Responsible for better arranging the periodic table by increasing ATOMIC NUMBER.

s and p.

-Good conductors of heat and electricity

-Malleable

-Ductible

-High tensile strength

-Have luster

-Poor conductors of heat and electricity

-Tend to brittle

-Gases at room temperature

Particle with a charge.

Positive ion

-Formed when electrons are lost.

Negative ion

-Formed when electrons are gained.

The physical and chemical properties of the elements are periodic functions of their atomic numbers.

One-half distance between two identical nuclei that are bonded. Increases going left and down.

The energy needed to remove the most loosely bound electron in an atom. Increases going right and up.

The ability of an atom in a chemical compound to attract (gain) electrons. Increases going right and up.

-Have properties of both metals and nonmetals.

-More brittle than metals, less brittle than most nonmettalic solids.

-Are semiconductors of electricity.

A mutual electrical attraction between the nuclei and valence electrons of different atoms that bind them together.

Transfer of electrons.

-Metal and nonmetal

Sharing of electrons.

-nonmetal and nonmetal

inversely proportional

Forces of attraction between molecules.

The negative region of one molecule is attracted to the positive region of another molecule.

A hydrogen atom that is boned to a highly electro-negative atom is attracted to an unshared pair of electrons of another highly electronegative atom on another molecule.

Intermolecular attractions resulting from the constant motion of electrons and the creation of instant dipoles.

Forces of attraction within atoms.

The smallest part of a covalently bonded substance within the properties of that substance.

(Valence shell electron pair repulsion). States that bonded atoms and unshared electron pairs orient themselves as far apart from each other as possible.

Bond in which bonded atoms have an unequal attraction for the shared electrons.

Bond in which bonding electrons are shared equally by bonded atoms.

Electrons NOT involved in a chemical bond.

The number of grams in one mole of a compound. A statement of the relative mass of each element contributes to the mass of the compound as a whole.

Formula that shows the whole-number ratio of elements in a compound.

The true numebr of atoms of each element in the formula compound.

1. Write the symbol and charge of the cation first.

2. Write the symbol and charge of the anion last.

3. If the value are opposite and equal, use NO SUBSCRIPTS!

4. If the values of the charges are different, Criss-Cross Method!

5. Never bring down a 1 it is understood.

6. The formula must be in the simplest ratio.

1. Write the cation name (metal) first.

2. Write the anion root name second.

3. Add “ide” to the end of the nonmetal element.

4. Use a Roman # for transition metals and Group IV cations. Except for Ag +1, Zn +2, Cd +2.

1. Write the least electronegative element first and most electronegative element last.

2. The prefix before the names of the elements tell the number of atoms for each element and the subscript use.

3. DO NOT USE CHARGES!!!!!!!

4. DO NOT CRISS-CROSS!

1. Do not use prefix on the first element if only one atom is present.

2. If more than one atom of the first element is present, use a prefix with it.

3. ALWAYS use a prefix before the second element’s name!

4. Add “ide” to the ending of the second element.

Hydro-nonmetal-ic.

-DON’T use the prefix hydro-

-Use the stem of the polyatomic and change the ending to…

1. -ate changes to -ic

2. -ite changes to -ous

A + X→AX

AX→A + X

A + BX → AX + B

AX + BY → AY + BX

Hydrocarbon + O2 → CO2 + H2O

F2, Cl2, Br2, I2, O2, N2, H2