Exam 2 PHS study guide

English

Based off of body parts, units, not systematically related

Metric system

Based off of seven base units, all other units derived from these (nature)

Four fundamental properties

Length, time, mass, charge

Metric prefixes

Represent small and large amounts by factors of 10

Density

How much matters packed into a given volume

Mass

The fundamental quantity matter that makes up an object

Volume

How much space something takes up

General scientific activity

Collect observations, develop, explanations, and test, explanations

Atomic number

number of protons

Atomic mass

Number of protons and neutrons

Isotopes

Many variations of the same elements same number of protons but different numbers neutrons

SI base units

meter (m), kilogram (kg), second (s), ampere (A), kelvin (K), mole (mol), candela (cd)

Quantum mechanics

Explains about wave, particle, duality, quantize, energy, explains what classical physics cannot, i.e. black body radiation

Mole

Avogadro's number 6.02x10^23

Quantitative use of equations

Molecular use of reactants and products. Mole ratios of reactants and products. Mass ratios of reactants and products.

Nomenclature rules ionic

1) Write symbol for positive ion first followed by negative ion symbol

2) assign subscripts to assure compound is electrically neutral

Nomenclature rules covalent

1) First element in formula named first with number indicated by Greek prefix

2) stem name of second element next Greek prefix for number ending in ied

How to read the periodic table

Each row is a period. Each vertical line is a family. The left side of the table is metals where the right side is not metals.

Chemistry

The study of matter and the changes undergoes

States of matter

Solid liquid gas aqueous

(s)

Solid

(l)

Liquid

like dissolves like

polar dissolves polar, nonpolar dissolves nonpolar

(g)

Gas

(aq)

aqueous

Monoatomic

One

Diatomic

Two

Triatomic

Three

Valance electrons

Outer electrons determine the chemical properties of an atom

Ionic bond

Electrons are given up to foreign either plus or minus ionic bond electrons are transferred

Covalent bond

Electrons are sharing, typically between nonmetals the right side of the periodic table

Empirical

Ionic in the simplest whole number

Molecular

Covalent, actual number in a compound

Formula weight

Number of atomic weight of atoms in a chemical formula

Percent composition of compounds

Finding the mass percent of an individual element from the weight

Balance equations

Change coefficients

Combustion reaction

A hydrocarbon in the presence of oxygen reacts to carbon dioxide and water

Combination reaction

A + B --> AB synthesis reaction in which two or more substance combined to form a single compound

Decomposition reaction

AB --> A + B a compound is broken down into simpler functions

Replacement reaction

An atom or polyatomic ion is replaced in a compound by a different atom or a polyatomic ion X+AB —-> XB+A

Ion exchange reaction

AX + BY --> AY + BX a reaction that takes place when the ions are one compounds interact with ions of another compound

Properties of water

1) universal solvent

2) solid phase less than than liquid

3) high specific heat

4)high latent heat of vaporization

5) all results from waters chemical structure

Water structure

Polar covalent bonding, oxygen negative center hydrogen two ends positive

Solution

Components of a solution solvent and solute

Solvent

Present in larger amounts

Solute

Components is often in solvent

Solubility

Concentration of saturated solution

Saturation

Solute dissolving limit

Miscible

Can mix an any proportions without separating

Immiscible

Do not mix

Soap

Has properties of both polar and nonpolar

Concentration ratios

Relative amounts of solute and solvent

Ppm

parts per million

ppb

parts per billion

percent by volume

V solute/ m solvent times 100% = % solute

Molarity

Moles of solute in 1 L of solution

Molarity equation

moles of solute/1L of solution

Concentrated

large amount of solute

Dilute

small amount of solute

Electrolytes

Solutions of bionic substances, conduct electricity

Non-electrolytes

Non-conductors sugar and alcohol solution

Ionization

Forming ions from molecules may occur as polar molecules

Normal Boiling point

Temperature where vapor pressure equals average sea level atmospheric pressure

Freezing point

Kinetic energy molecules reduce enough to allow crystallization

Properties of acids

Proton donor, change in color, neutralize bases

Properties of basis

Proton acceptor, reverse color, slippery on skin

PH scale

Pure water weekly ionized seven heaven, neutral, acid below seven, alkine above seven

Percent by weight

m solute / m solvent times 100% = solute

Hydroxide

OH-

Nitrite

NO2 charge -1

Nitrate

NO3 charge -1

Carbonate

CO3 charge -2

Sulfate

SO4 charge -2

Phosphate

PO4 charge -3

law of conservation of mass

atoms are neither created nor destroyed in chemical reactions

Functional groups

Responsible for chemical properties of organic compounds

Ketone

RCOR

Aldehydes

RCHO

Isomers

Compounds with the same formula but different structures.

Saturated

All carbons are bonded to max of four atoms

Unsaturated

All carbons are bonded to two or three atoms

Alkanes

a hydrocarbon containing only single covalent bonds (CnH2n+2)

Alkenes

Hydrocarbons with a double carbon carbon bond (CnH2n)

Alkynes

Hydrocarbons with a triple carbon carbon bond (CnH2n-2)

Ethers

ROR