CHEM 111 EXAM 1 Study Guide

length

meters (m)

mass

kilograms (kg)

time

seconds (s)

temperature

kelvin (K)

electric current

ampere (A)

amount of substance

mole (mol)

peta (P)

1,000,000,000,000,000 (10^15)

tera (T)

1,000,000,000,000 (10^12)

giga (G)

1,000,000,000 (10^9)

mega (M)

1,000,000 (10^6)

kilo (k)

1,000 (10³)

deci (d)

0.1 (10^-1)

centi (c)

0.01 (10^-2)

milli (m)

0.001 (10^-3)

micro (μ)

0.000001 (10^-6)

nano (n)

0.000000001 (10^-9)

pico(p)

0.000000000001 (10^-12)

femto(f)

0.000000000000001

atto(a)

0.000000000000000001 (10^-18)

Extensive

depend on amount of substance EX

Intensive

do not depend on the amount of substance EX

precision

repeatability

accuracy

closeness to actual target

law of conservation of mass

in a chemical reaction matter is neither created nor destroyed

law of definite proportions

all molecules of the same identity have the same ratios of atoms

law of multiple proportions

different molecules make from the same two elements exist in whole number ratio of their masses.

Electron

Outside of the nucleus; -1 charge; mass 1/1800 amu

neutron

inside the nucleus; no charge; mass 1 amu

Proton

inside the nucleus; +1 charge; mass 1 amu

Representative elements

main group of elements

Family 1

Alkali metals

Family 2

Alkaline earth metals

Family 3-12

Transition metals

Family 16

Chalcogens

Family 17

halogens

Family 18

Noble Gases

John Dalton

atomic theory states 1. Each element is composed of tiny, indestructible particles called atoms. 2. All atoms of a given element have the same mass and other properties 3. Atoms combine in simple whole number ratios to form compounds 4. Atoms of one element cannot change into atoms of another element… they can only change the way they are bound together with other atoms

JJ Thomson

discovered electrons and performed cathode ray experiments to determine the charge of the electron. He also proposed the plum pudding model and proposed that negatively charged electrons were small particles held within a positively charged sphere

Ernest Rutherford

used alpha particles to test plum pudding model...proposed nuclear theory, studied under Thomspon and believed the plum pudding model at the time of his experiments. Discovered that most of the atoms mass and all of its positive charge are contained in a small core known as the nucleus, that most of the volume of the atom is empty space throughout which tiny negatively charged particles known as electrons are dispersed, and that there are equal number of electrons and protons so that the atom is neutra