Chemistry- Atomic Theory/structure & Inorganic Compounds

Front 1

Dalton Atomic Model

Back 1

Elements are composed of particles called atoms, atoms of the same element are alike in mass and size, atoms of different elements have different mass and size, atoms combine to form compounds by the union of two or more atoms of different elements, atoms combine to form compounds in simple ratios, and atoms of two elements may combine in different ratios to form more than one compound.

Front 2

Law of Definite Composition

Back 2

A compound always contains two or more elements chemically combined in a definite proportion by mass.

Front 3

Law of Multiple Proportions

Back 3

Atoms of two ore more elements may combine in different ratios to produce more than one compound.

Front 4

Subatomic Particles

Back 4

Electrons, protons, neutrons.

Front 5

Electron

Back 5

(e-) A particle with negative charge (-1)
(Number of electrons for IONS = atomic number - the charge)
(If not ionic (no charge (pos. or neg.) number of electrons = number of protons)

Front 6

Proton

Back 6

A particle with mass and a positive charge (+1)
(Number of protons = atomic number)

Front 7

Neutron

Back 7

Neither positive or negative (neutral)
(Number of neutrons = mass number - atomic number)

Front 8

Thomson Model of the Atom

Back 8

Electrons are negatively charged particles embedded in the positively charged atomic sphere.

Front 9

The mass of an helium atom is 6.65 x 10 ^ -24 g. How many atoms are in a 4.0 g sample of helium?

Back 9

(4.0 g) x (1 atom He (Helium) / 6.65 x 10 ^ -24g) = 6.0 x 10 ^23 atoms He.

Front 10

Rutherford Gold Foil Experiment

Back 10

An experiment where small particles were shot at a thin sheet of gold. It was found that a small percentage of the particles were deflected, while a majority passed through the sheet.

Front 11

Atomic Number

Back 11

The number of protons in the nucleus of an atom.

(Atomic number = number of protons in the nucleus)

Front 12

Isotopes

Back 12

Atoms of an element having the SAME atomic NUMBER but DIFFERENT atomic MASSES.

Front 13

Mass number

Back 13

The sum of the number of protons and neutrons in the nucleus.

Front 14

Atomic mass unit (amu)

Back 14

A unit of mass equal to 1/12 of a carbon-12 atom.

Front 15

How many protons, neutrons and electrons are in this isotope?

mass number- 16
atomic number- 8
symbol- O

Back 15

protons = 8
electrons = 8
neutrons = 8

Front 16

How many protons, neutrons and electrons are in this isotope?

mass number- 80
atomic number- 35
symbol- Br

Back 16

protons = 35
electrons = 35
neutrons = 45

Front 17

How many protons, neutrons and electrons are in this isotope?

mass number- 235
atomic number- 92
symbol- U

Back 17

protons = 92
electrons = 92
neutrons = 143

Front 18

How many protons, neutrons and electrons are in this isotope?

mass number- 64
atomic number- 29
symbol- Cu

Back 18

protons = 29
electrons = 29
neutrons = 35

Front 19

Chlorine is found in nature as two isotopes:

mass - 37
atomic number - 17
symbol- Cl
percent abundance - 24.47%

-and-

mass- 35
atomic number -17
Same symbol
percent abundance - 75.53%

The atomic masses are 36.96590 and 34.96885 amu respectively. Find the average atomic mass of chlorine (Cl).

Back 19

(0.2447) x (36.96590 amu) + (0.7553) x (34.96885 amu)
= 35.46 amu (4 sig figs)

Front 20

Writing Ionic Compound Formulas

(Ex 1: Calcium Chloride)

Back 20

Ions= Ca 2+ and Cl-

-CRISS-CROSS-

Bring the (2+) to the Cl and the (-1) to the Ca

Therefore the formula = CaCl2 (The one does not need to be represented in formulas)

Front 21

Writing Ionic Compound Formulas

(Ex 2: Magnesium Oxide)

Back 21

Ions= Mg 2+ and O 2-

The (2-) from O neutralizes the (2+) from the Mg (Because 2 + -2 is 0)

Therefore the formula = MgO

Front 22

Writing Ionic Compound Formulas

(Ex 3: Barium Phosphide)

Back 22

Ions= Ba 2+ and P 3-

-CRISS CROSS-

Bring the (3-) from P to Ba and the (2+) from Ba to P (Not the charges; just the number)

Therefore the formula = Ba3P2

Front 23

Writing Binary Compounds of Metal Forming One Type of Cation

Back 23

1st) Write the name of the Cation.
2nd) Write the suffix (ide) for the suffix.

(Ex: CaBr2 = Calcium BromIDE |Li2O = Lithium OxIDE)

Front 24

Writing Binary Compounds Contaning a Metal That Can Form 2 or More Types of Cations:


Ca 2+ and Br 1-

Back 24

= CaBr2

Front 25

Write the Ionic Compound Formula for:

Mg 2+ and N 3-

Back 25

= Mg3N2

Front 26

Writing Binary Compounds Contaning a Metal That Can Form 2 or More Types of Cations:

Back 26

1st) Write the name of the cation.
2nd) Write the charge of the cation as ROMAN NUMERAL In parentheses.
3rd) Write the stem of the anion and add the suffix (ide).

Front 27

Writing Binary Compounds Contaning a Metal That Can Form 2 or More Types of Cations:

(Ex: FeCI2)

Back 27

Fe (Iron) Cl (Chlorine)

Fe (2+ charge) Cl (1- charge)

Fe (2+ charge) = Roman numeral (II)

Formula = Iron (II) ChlorIDE

Front 28

Name this Binary Ionic Compound:

FeCI3

Back 28

= Iron (III) Chloride

Front 29

Name this Binary Ionic Compound:

CuCI

Back 29

= Copper (I) Chloride

Front 30

Write the formula for this compound:

Tin (IV) Chromate

Back 30

= Sn (CrO4)2

Front 31

Write the formula for this compound:

Chromium (III) Bromide

Back 31

= CrBr3

Front 32

Naming Binary Compounds Containing 2 Nonmetals

(Ex: PCl 5-)

Back 32

1st) Write the name of the first element using a prefix if there is more than one atom of the element.
2nd) Write the stem of the second element and add the suiffix (ide). Use a prefix to indicate the number of atoms for the second element. (E.g. (in numerical order) mono, di, tri, tetra, penta, hexa, hepta, octa, nona, deca...)

PCI 5- = Phosphorus PENTAchlorIDE

Front 33

Name this Binary Compound:

SO2

Back 33

= Sulfur Dioxide

Front 34

Name this Binary Compound:

N2O5

Back 34

= Dinitrogen Pentoxide