Midterm 1 Gen Chem 1

anything that has mass and takes up space

matter

has distinct properties and a composition that does not vary from sample to sample

substances

2 types of substances

element and compound

substance that cannot be decomposed into simpler substances

element

• can be decomposed into smaller substances and is made up of more than one element

• have a definite composition, meaning the number of atoms of each element in it is the same from sample to sample

compound

building block of matter

atom

• made up of substances

• can vary in composition throughout a sample

mixtures

have the same composition throughout a sample (aka a soulution)

homogenous mixture

varys throughout a sample

heterogenous mixture

can be observed without changing a substance into another substance

• color oder, density, melting point, boiling point, hardness

physical property

can only be observed when a substance is changed into another substance

• flammability/ ability to burn in oxygen

chemical property

quantity independent (boiling point, melting point)

• density, boiling point, color

intensive properties

quantity dependent (ex. mass, volume)

extensive properties

solid substances are separated form liquids and solutions

filtration

uses differences in boiling points to separate a liquid mixture into its components

distillation

technique that separates by differences in adhering to the solid phase

chromatography

Conversion between kelvin and celsius (0 K is absolute 0)

K = degrees C + 273.15

1. each element is composed of extremely small particles called atoms

2. All atoms of a given element are identical, but the atoms of one element are different form the atoms of all other elements

3. atoms of one element can not be changed created or destroyed

4. Compounds are formed when atoms of more than one element combine

Daltons atomic theory

Compounds have a definite composition, meaning that the relative number of atoms of each element in the compound is the same in any sample (Joseph Proust)

Law of constant composition

The total mass of substances present at the end of a chemical process are the same as the mass of the substances present before the process took place (Antoine Lavoiser)

Law of conservation of mass

If two elements, A and B form more than one compound the masses of B that combine with a given mass of A are in the ration of small whole numbers (Dalton)

Law of multiple proportions

Streams of negatively charged particles were found to emanate from cathode tubes causing fluorescence

Cathode ray experiment

importance of cathode ray experiment and who did it?

discovery of the electron JJ Thomson (1897)

Millikan Oil-Drop Experiment

purpose of Millikan Oil-Drop Experiment and who did it?

found charge of a single electron Robert Millikan (1909)

who discovered radioactivity?

Marie Curie

plum pudding model - JJ Tompson

what did the gold foil experiment find and who discovered it?

nucleus, Ernest Rutherford

proton charge

+1

neutron charge

0

electron charge

-1

the number of protons in the nucleus

atomic number

12

6 C top number?

mass number (protons + neutrons)

12

6 C bottom number

atomic number (number of protons/electrons)

atoms of the same element with different masses

Isotopes

Average of mass of all isotopes?

atomic weight (on periodic table)

name of columns on periodic table

groups

rows on periodic table

periods

pink

alkali metals

orange

alkaline earth metals

green

Chalogens

green/blue color

halogens

dark blue

noble gasses

where are non metals on periodic table other than hydrogen

right side

where are metalloids on periodic table?

stairs next to metals

where are metals?

on left side of the periodic table

Seven elements that occur naturally at diatomic molecules

Hydrogen, Nitrogen, Oxygen, Fluorine, Chlorine, Bromine, Iodine

the lowest whole-number ration of atoms of each element in a compound

empirical formula

the exact number of atoms of each elements in a compound

molecular formulas

when an atom gains/loses and electron

ion

formed when one electron is lost (pawsitive)

cation

formed when at least one electron is gained

anion

generally formed between metals and nonmetals

ionic compounds

charge of Ag (Silver)

1+

charge of Zn (Zinc)

2+

Charge of Cd (Cadmium)

2+

Charge of Al (aluminum)

3+

how to name ions from group 1 and group 2 and exceptions (Ag, Cd, Zn, Al)

element name + ion

NH4+

Amonium ion

H3O+

Hydronium

Co 2+

Cobalt(II) Ion

naming anions in groups15 16 and 17 rule?

start of name + ide

OH-

Hydroxide

CH3COO 2-

Acetate

CO3 2-

Carbonate

NO3 -

Nitrate

PO4 3-

Phosphate

SO4 2-

Sulfate

ClO3 -

Chlorate

CLO4 -

perchlorate

ClO2 -

chlorite

ClO -

Hyperchlorite

same formula but different structures

isomers