Fundamentals Of Chemistry Test 3

Front 1

GAS EVO REACTION:
Reactant type - Sulfides
Intermediate - ____
Gas Evolved - _____

Back 1

Gas evolved - H2S
Intermediate - None

EX: 2HCl (aq) + K2S (aq) ---> H2S(g) + KCl(aq)

Front 2

GAS EVO REACTION:
Reactant type - Carbonates & Bicarbonates
intermediate - ____
Gas Evolved - ____

Back 2

Gas evolved - CO2
Intermediate - H2CO3

EX: 2HCl(aq) + K2CO3(aq)----> H2O(l) + CO2(g) + 2KCl(aq)

Front 3

GAS EVO REACTION:
Reactant type - Sulfites & Bisulfites
Gas Evolved -_____
Intermediate - ____

Back 3

Gas evolved - SO2
intermediate - H2SO3

EX: 2HCl(aq) + K2SO3(aq)-----> H2O(l) + NH3(g) + KCl(aq)

Front 4

GAS EVO REACTION:
Reactant type - Ammonium
Gas Evolved - _____
intermediate - _____

Back 4

Gas evolved - NH3
Intermediate - NH4OH

EX: NH4Cl(aq) + KOH(aq) -----> H2O(l) + NH3(g) + KCl(aq)

Front 5

What are the 7 strongest acids? (all others are considered "weak")

Back 5

Hydrochloric acid
Hydrobromic acid
Nitric Acid
Sulfuric Acid
Hydroiodic Acid
Perchloric Acid
Acetic Acid

Front 6

What's the chemical formula for Hydrochloric acid?

Back 6

HCl

Front 7

Whats the chemical formula for Hydrobromic acid?

Back 7

HBr

Front 8

Whats the chemical formula for Nitric Acid?

Back 8

HNO3

Front 9

Whats the chemical formula for Sulfuric Acid?

Back 9

H2SO4

Front 10

Whats the chemical formula for Perchloric acid?

Back 10

HClO4

Front 11

Whats the chemical formula for Acetic Acid?

Back 11

HC2H3O2

Front 12

What are the 6 strongest bases? (all other bases are considered "weak")

Back 12

Sodium Hydroxide
Lithium Hydroxide
Potassium Hydroxide
Calcium Hydroxide
Strontium Hydroxide
Barium Hydroxide

Front 13

Compounds containing the following Ions are ALWAYS SOLUBLE:........

Back 13

Li^+
Na^+
K^+
NH4^+
NO3^-
C2H3O2^-

Front 14

If CO3^2- & PO4^3- are found in a compound they are always INSOLUBLE UNLESS they are paired with........

Back 14

Li^+, Na^+, K^+, NH4^+

Front 15

A _______ equation is a chemical equation showing the complete, neutral formulas for every compound in a reaction.

Back 15

Molecular equation

Front 16

A ________ equation is a chemical equation showing all of the species as they are actually present in solution.

Back 16

Complete Ionic equation

Front 17

A ________ equation is an equation showing only the species that actually participate in the reaction.

Back 17

Net Ionic equation

Front 18

________ reactions (also called neutralization reactions) generally form water and an ionic compound—called a salt—that usually remains dissolved in the solution

Back 18

Acid-Base Reactions

Front 19

______ reactions are characterized by the reaction of a substance with O2 to form one or more oxygen-containing compounds, often including water. Compounds containing carbon and hydrogen or carbon, hydrogen, and oxygen always form H2O and CO2 upon completion.

Back 19

Combustion reactions

Front 20

In a precipitation reaction, only _____ compounds form precipitates.

Back 20

Insoluble

Front 21

The fundamental definition of OXIDATION is the ____ of electrons.

Back 21

Loss of electrons

Front 22

The fundamental definition of REDUCTION is the _____ of electrons.

Back 22

Gain of electrons

Front 23

Oxidation-Reduction reactions (redox) involve a transfer of electrons. Many redox reactions involve the reaction of a substance with ____. Oxidation and reduction must occur _________. If one substance loses electrons (oxidation), then another substance must gain electrons (reduction).

Back 23

Involve O2

Must occur TOGETHER

Front 24

When an aqueous reaction forms a gas product, it's classified as a ________ reaction.

Back 24

Gas evolution reaction

Front 25

Greenhouse gases act like _______in a greenhouse.

Back 25

Glass

Front 26

The world's annual fossil fuel consumption shows that ___ mols of CO2 are produced for every ____ mols of octane (C8H18) burned.

Back 26

16 mols of CO2 for every 2 mols of octane (C8H18)

Front 27

If we know the worlds annual fossil fuel consumption, we can estimate the worlds annual ___ production.

2C8H18(l) + 25O2(g) ---> 16CO2(g) + 18H2O(g)

Back 27

CO2 production

Front 28

percent yield = _______ X 100%.

Back 28

Actual yield
-------------------------
Theoretical Yield

Front 29

_____ yield is the amount of product that can be made in a chemical reaction based on the amount of the limiting reactant.

Back 29

theoretical yield

Front 30

Amount of thermal energy emitted or absorbed by a chemical reaction, under conditions of constant pressure (which are common for most everyday reactions), can be quantified with a function called ______.

Back 30

Enthalpy

Front 31

An endothermic reaction (thermal energy flows into reaction from surroundings) has a sign of ___.

Back 31

(delta)H+

Front 32

An exothermic reaction (thermal energy flows out of the reaction into it's surroundings) has a sign of __.

Back 32

(delta)H-

Front 33

_____ yield is the amount of product that's actually produced by a chemical reaction.

Back 33

actual yield

Front 34

the _________ is the reactant that is completely consumed in a chemical reaction.

Back 34

limiting reactant

Front 35

Light is a form of __________.

Back 35

Electromagnetic radiation

Front 36

________ (ν) is defined as the number of cycles or crests that pass through a stationary point in one second.

Back 36

Frequency

Front 37

a _____ is A particle of light; a single packet of light energy.
-amount of energy of a _____ depends on wavelength

Back 37

Photon

Front 38

In the early twentieth century the quantum-mechanical model replaced Bohr orbits are replaced with quantum-mechanical _____.

Back 38

Orbitals

Front 39

In the quantum-mechanical model each orbital is represented by:
- a number called the principal ___________ which specifies the principal shell
- a _____ called the subshell which specifies the orbital shape

Back 39

Principle Quantum Number (n)

Letter

Front 40

The letters for subshells are:

Back 40

S - stupid
P - People
D - Die
F - First

Front 41

What are the total # of orbitals for:
S-
P-
D-
F-

Back 41

S - 1
P - 3
D - 5
F - 7

Front 42

What are the total number of electrons for the following:
S-
P-
D-
F-

Back 42

S - 2
P - 6
D - 10
F - 14

Front 43

What is the shape of the following:
S-
P-
D-
F-

Back 43

S - Sphere
P - Peanut
D - 4 leaf clover
F - Flower

Front 44

The __ orbital consists of the 1a & 2a columns on the periodic table

Back 44

S

Front 45

The __ orbital consists of the elements to the right of the transition metals on the periodic table.

Back 45

P

Front 46

The __ orbitals consist of the transition metals on the periodic table.

Back 46

D

Front 47

____ rule states that when filling orbitals of equal energy, electrons fill them singly first, with parallel signs.

Back 47

Hund's rule

Front 48

Whats the chemical equation for Strontium Hydroxide?

Back 48

Sr(OH)2

Front 49

Whats the chemical equation for Hyrdoiodic Acid?

Back 49

HI

Front 50

____rays and ____ rays are sometimes called ionizing radiation because the high energy in their photons can ionize atoms and molecules

Back 50

X-Rays
Gamma Rays

Front 51

ROYGBIV is in _____ order of energy (frequency (v))

Back 51

ascending

Front 52

Whats the chemical formula for Iodate?

Back 52

IO3^-

Front 53

What atoms can S^2- & OH^- be paired with and still be soluble?

Back 53

Ca 2+
Sr2+
Ba2+

Front 54

What is a property of a strong electrolyte solution?

Back 54

substances completely dissociate into ions in solution

Front 55

wavelength and frequency are _____ related.

Back 55

Inversely

Front 56

The rays of the electromagnetic spectrum in order of ascending wavelength (descending energy & frequency) is......

Back 56

Gamma
X
UV
Visible
Infrared
microwaves
radio waves

Front 57

the formula for displacement is...

Back 57

A + BC ------> AC + B

Front 58

the formula for synthesis or combination is.....

Back 58

A + B ------> AB

Front 59

The formula for double displacement is....

Back 59

AB + CD ------> AD + CB