Chem 151Aa Exam 1

Front 1

What is chemistry

Back 1

The study of matter and the change of matter

Front 2

Properties of each physical state of matter

Back 2

Solid:Has both definitive shape and definitive volume.

Gas:No fixed volume or shape, conforms to the shape of the container, can be compressed to smaller volume or expanded to occupy larger volume

Liquid:Distinct volume independent of its container but has no specific shape.

Front 3

The Seven Diatomic Elements

Back 3

*Don't forget that it looks like a 7 on the periodic table*

Hydrogen

Nitrogen

Oxygen

Fluorine

Chlorine

Bromine

Iodine

Front 4

What is an Element

Back 4

A substance that cannot be chemically decomposed into a simpler substance..

Front 5

What are atoms

Back 5

Atoms are the smallest building blocks of matter. Some examples are Helium, Iron, and hydrogen

Front 6

What are Molecules

Back 6

Two or more atoms are joined together in a specific shape. A water molecule H2O, is an example of a molecule.

Front 7

Extensive and intensive changes.

Back 7

Intensive properties are related to the physical properties of matter. Intensive properties do not depend on the amount of matter present. I.E Color, luster, odor, hardness, boiling point, conductivity...etc

Extensive properties are related to the amount of matter present. The mass, weight, length, and volume fall under this category

Front 8

The 4 common SI units

Back 8

Length: Meters

Mass: Kilograms

Temperature: Kelvin

Time: Seconds

Front 9

Common Metric Prefixes and meanings

Back 9

http://www.radioing.com/eengineer/metric.gif

Front 10

What are the two derived units?

Back 10

Volume: Length x Height x Width

Density: The amount of mass in a unit volume of a substance.

D= (M / V) Mass over volume

Front 11

What are Exact Numbers and Inexact numbers

Back 11

Exact numbers have no uncertainty. Examples are, conversion factors, or counting items.

12 eggs in a dozen

1000g = 1Kg

100cm= 1m

Inexact numbers have some uncertainty. This is obtained from measurement. Error always exists in measured quantities

Front 12

Sig Fig Help

Back 12

1. All nonzero digits are significant. (2.23 g = 3 SF)

2. Zeroes between two significant figures are themselves significant. (1005 kg = 4 SF)

3. Zeroes at the beginning of a number are never significant. (0.0200 g = 3 SF)

4. Zeroes at the end of a number are significant if a decimal point is written in the number.

Front 13

Temperature conversions

Back 13

K= C + 273.15

C= 5/9(F - 32)

F= 9/5 (C) + 32

Simplified: 9(c)=5(F) - 160

Front 14

Dalton's Atomic Theory

Back 14

The postulates are;

1) Each element is composed of extremely small particles called atoms.

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

3) Atoms of one element cannot be changed into atoms of a different element by chemical reactions; atoms are neither created nor destroyed in chemical reactions.

4) compounds are formed when atoms of more than one element combine; a given compound always has the same relative number and kind of atoms.

Front 15

Law of Constant Composition

Back 15

In any given compound the relative numbers and kind of atoms are constant

Front 16

Law of Conservation of Mass

Back 16

The total mass of materials present after a reaction is the same as the total mass present before reaction.

Front 17

Law of Multiple Proportions

Back 17

If two elements, A & B combine to form more than one compound, the masses of B that can be combined with a given mass of A are in a ratio of small whole numbers

Front 18

What Experiments lead to the discovery of atomic structure.

Back 18

Thomson's Cathode Ray Experiments

Millikan's Oil drop Experiments

Rutherford's Experiments

a) Radiation Experiments

b) Gold Foil Experiment

Front 19

JJ Thomas info

Back 19

He used a magnet and a cathode ray in order to prove the existence of electrons

Front 20

Millikan's oil-drop

Back 20

Used Thomson's charge to mass ration to calculate the mass of an electron. Observed oil droplets suspended due to magnetism.

Charge of an electron: 1.602 x 10^(-19)

Mass of an Electron: 9.10 x 10^(-28)

Front 21

Rutherford Experiments

Back 21

Rutherford shot alpha particles at gold and some bounce back instead of going forward. Discovered the nucleus. used radiation to determine 3 types of radiation. Alpha Beta and Gamma

Front 22

Particles

Back 22

Proton Positive 1.0073

Neutron None 1.0087

Electron Negative 5.486 x 10^(-4)

Front 23

Periodic Law

Back 23

Certain elements can be groupedtogether by their similar physical appearance,properties, and chemical behavior

Front 24

Molecular (Covalent) Compounds

Back 24

Composed of molecules formed by atoms of two or nonmetal elements (No2). Electrons are shared to form covalent bonds.

Front 25

Ionic Compounds

Back 25

Compound composed of cations and anions combined in rations, yielding an electrically neutral substance. Electrons are transferred

Front 26

Periodic table groups

Back 26

Alkali metals

Alkali earth metals

Transition Metals

Pnictogens

Chalcogens

Halogens

Noble gasses

Front 27

Cation Vs Anion

Back 27

cations are positively charged ^+ +^

+

Anions are negatively charged

Front 28

Avogadro's #

Back 28

6.02 x 1023 objects per 1 mole

Front 29

Practice Percent Composition

Front 30

Practice Conversions with moles

Front 31

Explain the relationship between moles, mass, and number of atoms or molecules

Back 31

When i say moles you say grams. The relationship between a mole and mass is Avogadro'sumber. It takes a theoretical amount of an atom or molecule and allows us to convert it into a measurable quantity.