Chem 1401 (Exam 1)

Solid

Definite shape and volume

liquid

A state of matter that has no definite shape but has a definite volume.

gas

A state of matter with no definite shape or volume

Mass

the amount of matter in an object

Weight

A measure of the force of gravity on an object

extensive property

a property that depends on the amount of matter in a sample

intensive property

a property that depends on the type of matter in a sample, not the amount of matter

physical property

A characteristic of a pure substance that can be observed without changing it into another substance

chemical property

A characteristic of a pure substance that describes its ability to change into different substances

formation of rust

chemical change

separation of paint

physical change

cooking an egg

chemical change

melting a popsicle

physical change

combustion of gasoline

chemical change

Blood

heterogeneous

orange juice with pulp

heterogeneous mixture

Air

heterogeneous mixture

Helium

pure substance

Gasoline

homogeneous mixture

Ramen noodle soup

heterogeneous mixture

Pure salt in water

Homogeneous

There are about ______ elements in nature

90

Sodium (Na)

Natrium

Gold (Au)

Aurum

Lead (Pb)

Plumbum

Many elements were not discovered until

18th and 19th centuries

artificial elements were created until

19 centuries

diatomic elements

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

Monoatomic elements

most of the elements, exist as single atoms

polyatomic molecule

a molecule that consists of more than two atoms

Have No Fear Of Ice Cold Beer

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

Compunds

form when two or more elements combine chemically

CH4

Methane (natural gas)

H2O

Chemical formula for water

C6H12O6

chemical formula for glucose(sugar)

AgCl

silver chloride

NaBr

sodium bromide

P4

Phosphorus

S8

Sulfur

Na

Sodium

ionic bond

metal + nonmetal

covalent bond

nonmetal + nonmetal

Mass unit

kilogram (kg) or gram (g)

length unit

meter (m)

Time unit

seconds (s)

temperature unit

Kelvin (K)

amount of substance unit

mole (mol)

electric unit

ampere (A)

luminous intensity unit

candela (cd)

Tera-

10^12

Giga-

10^9

Mega-

10^6

kilo-

10^3

deci

10^-1

centi

10^-2

milli

10^-3

micro

10^-6

nano

10^-9

pico

10^-12

femto

10^-15

atto

10^-18

zemto

10^-21

cm^3

mL

cubic centimeter

mL

dm^3

L

Celcius

(F-32) x 5/9

Kelvin

C + 273.15

Fahrenheit to Celsius

C=5/9(F-32)

water boils

100 C and 212 F

significant figures

all the digits in a measurement that are directly measured, plus the last digit, which is estimated

1in

2.54cm

1lb

454.59g

gas chromatography/mass spectrometry (GC/MC)

Provides greatest specificity and utmost sensitivity for drug testing

law of definite proportions

a given compound always contains exactly the same proportion of elements by mass

the law of constant composition

A given compound always contains elements in exactly the same proportion by mass

Law of Conservation of Mass

Matter is not created nor destroyed in any chemical or physical change

Law of Multiple Proportions

if two or more different compounds are composed of the same two elements, then the ratio of the masses of the second element combined with a certain mass of the first element is always a ratio of small whole numbers

Earnest Rutherford

Gold foil experiment. Said the atom is mostly empty space. Discovered the nucleus.

mass number

protons + neutrons

atomic number

number of protons

Isotopes

Atoms of the same element that have different numbers of neutrons

atomic weight

% x mass isotope 1 & 2

Molecule

A group of atoms bonded together

Compound

A substance made up of atoms of two or more different elements joined by chemical bonds

empirical formula

a chemical formula showing the ratio of elements in a compound rather than the total number of atoms

spatial isomers

compounds in which the relative orientation of the atoms in space differ

Mercury Hg

liquid at room temp.