Chemistry 10 Boczany 1

Front 1

What is matter?

How do you classify matter as a pure substance, compound, heterogeneous mixture, homogeneous mixture?

Back 1

Matter is anything that has mass and occupies space.

Pure substances have a fixed composition and a unique set of properties. Compounds are pure substances that contain more than one element. Heterogeneous are nonuniform mixtures where composition varies. Homogeneous are uniform where it has the same composition.

Front 2

Separation techniques?

Back 2

Filtration: used to separate a heterogeneous solid-liquid mixture;passed through a barrier w/fine pores (filter paper)
Distillation: separates homogeneous solid-liquid mixture;liquid vaporizes, leaving a residue of the solid in the distilling flask
Chromatography: separates all mixtures
Gas-Liquid Chromatography: mixture of volatile liquids and gases are introduced into one end of a heated gas tube
Decant: pour off the dense liquid

Front 3

Qualitative vs. Quantitative

Back 3

qualitative: description
quantitative: number/amount

Front 4

Precision vs. Accuracy

Back 4

accuracy: closer to true value
precision: reproducibility no matter how true to value

Front 5

Scientific Notation

Back 5

C x 10^n
shorter way of writing large numbers

Front 6

What are SI units, prefixes, and their values?

Back 6

Uses the Metric System
based on increments of 10
length:meter(m)
volume: cubic centimeters, liters, milliliters (cc, L, mL)
mass:kilograms(Kg)
time:second(s)
amount: moles(mol)
temperature: Kelvin(K)
electrical current: ampere(A)
luminous intensity:candela(cd)

K(kilo)H(hecto)D(deca)b(base)d(deci)c(centi)m(milli)..n(nano)..|u(m, mu)

Front 7

Convert degrees C/F to degrees K

Back 7

C--> 5/9 (F-32)
F-->9/5C+32
K-->C+273.15 (true measure, no degrees for Kelvin)

Front 8

Significant Figures

Back 8

1) non-zero numbers are significant
2)zero's between significant figures are also significant
3)zero's at the end of a number RIGHT of the decimal are significant
4)zero's at the end of a number LEFT of the decimal are NOT significant (place holders)
5)all zeros before the first non-zero number are NOT significant (place holders)
6)count has an infinite number of significant figures or zero significant features (ex. 115 cars)

Front 9

density calculations

Back 9

d=m/v
m=(d)(v)
d=(m)(v)

Front 10

conversion factor

Back 10

given x want/given = want

Front 11

Physical vs. Chemical Changes

Intensive vs. Extensive Changes

Back 11

phys:a change in a substance that does not involve a change in identity of a substance
chem:a change in which one or more substances are converted into different substances

inten:independent on the amount ex. boiling point
exten:dependent on the amount ex. mass

Front 12

Law of Conservation of Matter

Back 12

mass cannot be created not destroyed

Front 13

Law of Constant Composition (Definite Proportions)

Back 13

regardless of amount, compound has same elements in the same properties by mass

Front 14

Law of Multiple Compositions

Back 14

Same elements can be in different ratios to create different compounds
ex. carbon dioxide & carbon monoxide

Front 15

John Dalton - 1808 - Atomic Theory

Back 15

1) All matter is composed of atoms
2)Atoms of the same element are identical in size, mass, and other properties; atoms of different elements differ in their properties
3)Atoms cannot be subdivided, created or destroyed
4)Atoms of different elements combine in simple ratios t0 form chemical compounds (H20)
5)In chemical reactions, atoms are combined, separated, and rearranged

Front 16

Modern Atomic Theory

Back 16

The discovery of subatomic particles that make up atoms
The discovery of isotopes

Front 17

Protons
Electrons
Neutrons

Back 17

+ | inside the nucleus
- |in the electron cloud (orbitals)
no charge | inside nucleus

Front 18

Atomic Number

Back 18

The number of protons in the nucleus of each atom, this never changes

Front 19

Atomic Mass Number

Back 19

The number of protons and neutrons in the nucleus of the atom

Front 20

Isotopes (nucleotides)

Back 20

Atoms of the same element that differ in number of neutrons in the nucleus, hence they have different masses

Front 21

Ions

Back 21

When you lose or gain electrons
Cations: +, loses e-
Anions: -, gains e-

Front 22

J.J. Thompson - Late 1800s

Back 22

Discovered the electron, used a cathode ray tube to deduce presence of a negatively charged particle.

Front 23

Earnest Rutherford - Early 1900s

Back 23

Student of Thompson; found that most particles were passed through, few were slightly deflected, very few were greatly deflected

Front 24

Rutherford Atomic Model

Back 24

Front 25

Neils Bohr - Early 1900s

Back 25

Student of Rutherford; as you get higher in the levels., the areas are closer

Front 26

Bohr's energy levels

Back 26

Front 27

Erwin Schrödinger - 1900s

Back 27

Quantum Mechanical Model
Mathematical model of the atom; an electron cloud is a volume of space where an electron COULD be located

Front 28

Robert Milikan

Back 28

discovered the mass of an electron and charge
mass of e-=1/1840 H atom
1 negative charge

Front 29

James Chadwick - 1932

Back 29

discovered the neutron(has no charge)