"Advanced Chemistry 10 - Summary of Semester #1"

Accuracy

The agreement of a particular value with the true value.

Precision

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

Direct Proportion

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

\-Straight Line

Inverse Proportion

Two quantities where their product is constant.

\-Curve Line

SI

Le Systeme International d’Unites

Derived Unit

Combinations of SI base units

Quantitative

Numerical information

Qualitative

Non-numerical information

Scientific Notation

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

For electronic devices…

record all digits.

For non-electronic devices..

read all certain digits and one uncertain digit.

Significant Digits

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

Atlantic

Decimal absent (right).

Pacific

Decimal present (left).

When adding or subtracting decimals…

use the fewest number of decimal places.

When multiplying or dividing decimals…

use the least amount of significant digits.

Dimensional Analysis

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

Denisty

Mass/Volume

\-directly proportional

Thomson

Discovered the electron (cathode ray tube)

Millikan

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

Rutherford

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

Bohr

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

Avogadro

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

Law of Conservation of Mass

Mass is neither created nor destroyed.

Law of Definite Proportions

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.

Law of Multiple Proportions

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.

Dalton’s Theory

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.

Nucleus

Center of the atom

Protons

Positive charge

Neutron

Neutral charge

Electron

Negative charge

Atomic Number

Number of protons. Shown on the periodic table.

Mass Number

Protons + Neutrons

Isotopes

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

Molar Mass

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

Avogadro’s Number

6\.022x10^23

Electrons have properties of both …

particles and waves.

Wavelength

Distance between two consecutive corresponding points on a wave.

Frequency and energy are …

Directly proportional

Frequency

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

Ground state electron

Lowest energy state.

Excited state electron

Highest energy state.

The emission of light is funamentally related to the behavior of the …

electrons.

Heisenberg uncertainty principal

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

Schrodinger

The quantum theroy.

DeBrogile

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

Quantum Numbers

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

Aufbau Principle

Electrons enter the lowest energy level possible

Pauli Exclusion Principle

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

Hund’s Rule

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

Octet Rule

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

Photons

Particles of light. Discovered by Einstein.

Quantum Leap

A huge, often sudden, increase or advance.

When an electron returns to the ground state from excited, it ...

releases the excess energy.

Principal Quantum Number

Describes the size of orbital.

Angular Momentum Quantum Number

Describes the shape of the sublevel.

Magnetic Quantum Number

Describes the orientation about the azes.

Spin Quantum Number

Describes the rotation of an electron.

Mendeleev

Responsible for arranging the periodic table by increasing ATOMIC MASS.

Moseley

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

Main group elements

s and p.

Metals

\-Good conductors of heat and electricity

\-Malleable

\-Ductible

\-High tensile strength

\-Have luster

Nonmetals

\-Poor conductors of heat and electricity

\-Tend to brittle

\-Gases at room temperature

Ion

Particle with a charge.

Cation

Positive ion

\-Formed when electrons are lost.

Anion

Negative ion

\-Formed when electrons are gained.

Periodic Law

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

Atomic Radius

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

Ionization Energy

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

Electronegativity

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

Metalloids

\-Have properties of both metals and nonmetals.

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

\-Are semiconductors of electricity.

Chemical Bond

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

Ionic Bond

Transfer of electrons.

\-Metal and nonmetal

Covalent Bond

Sharing of electrons.

\-nonmetal and nonmetal

Bond energy and bond length are …

inversely proportional

Intermolecular Forces

Forces of attraction between molecules.

Dipole-Dipole

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

Hydrogen Bonding

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.

London Dispersion Forces

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

Intramolecular Forces

Forces of attraction within atoms.

Molecule

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

VSEPR Theory

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

Polar Covalent

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

Non-polar Covalent

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

Lone Pairs

Electrons NOT involved in a chemical bond.

Percent Composition

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.

Empirical Formula

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

Molecular Formula

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

Writing Binary Ionic Compounds

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.

Naming Binary Ionic Compounds

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.

Writing Binary Covalent Compounds

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!

Naming Binary Covalent Compounds

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.

Naming Binary Acids

Hydro-nonmetal-ic.

Naming Ternary Acids

-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

Synthesis

A + X→AX

Decomposition

AX→A + X

Single Replacement

A + BX → AX + B

Double Replacement

AX + BY → AY + BX

Combustion

Hydrocarbon + O2 → CO2 + H2O

Diatomic Elements

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