Final study Guide Flashcards
(97 cards)
0
Q
- the oxidation number of atoms in a compound must equal zero
- the sum of the oxidation number in polyatomic ions is zero
- alkali metals have the oxidation number +1.
- an ions charge is equals to its oxidation number
Which one isn’t true.
A
The sum of the oxidation number in polyatomic ions is zero
1
Q
What is a compound that contains a water molecule in its crystalline structure?
A
Hydrates
2
Q
The Greek prefixes system is normally used for either ionic or covalent compounds. T/F
A
False
3
Q
What is a compound that contains hydrogen, oxygen, and another nonmental?
A
Ternary acid
4
Q
What is the oxidation number of H in MgH2.
A
-1
5
Q
The prefix hepta- means
A
7
6
Q
Name the following compound: P2O5
A
Diphosphorous pentoxide
7
Q
Write a chemical formula for the following compound: ammonium fluoride
A
NH4F
8
Q
What represents the number of electrons that an atom in a compound must gain or lose to return to its neutral state?
A
Oxidation number
9
Q
What is the oxidation number of Cu in CuSO4?
A
+2
10
Q
System for naming compounds
A
Nomenclature
11
Q
Another name for stock system which indicates the oxidation number used of the metal in the ionic compound
A
Roman numeral system
12
Q
Covalently bonded groups of atoms that carry a charge
A
Polyatomic atoms
13
Q
The number of electrons that an atom in a compound must gain or lose to return to its neutral state
A
Oxidation number
14
Q
A compound that is not ionic or an acid
A
Binary covalent compound
15
Q
Acids consisting of hydrogen and one other nonmetal
A
Binary acid
16
Q
Anions that contain oxygen and one other element
A
Oxyanions
17
Q
Indication of how many atoms of each element are in a binary covalent compound
A
Greek prefix system
18
Q
The more electronegative element receives a negative oxidation number, and a less electronegative element receives a positive oxidation number. T/F
A
False
19
Q
The sum of the oxidation number of all the atoms in a compound must equal zero. T/F
A
True
20
Q
Group one has what oxidation number?
A
+1
21
Q
What is the oxidation number of halogens typically have when they bond with metals?
A
-1
22
Q
What is the oxidation number of P in Cu3P2?
A
-3
23
Q
What is the oxidation number of Hg3(PO4)2?
A
+2
24
Identify the name for the following compound: Pb(NO3)2
Lead (II) nitrate
25
Identify the name for the following compounds: KClO3
Potassium Chlorate
26
Identify the name for the following compounds: MgSO4 x 7H2O
magnesium sulfate heptahydrate
27
Write the correct chemical formula for the following compound: potassium cynide
KCN
28
Write the correct chemical formula for the following compound: aluminum phosphate
AlPO4
29
Write the correct chemical formula for the following compound: ammonium fluoride
NH4F
30
Write the correct chemical formula for the following compound: sodium phosphate
Na3PO4
31
Write the correct chemical formula for the following compound: aluminum and chlorine
AlCl3
32
Write the correct chemical formula for the following compound: potassium and oxygen
K2O
33
Write the correct chemical formula for the following compound: hydrogen and bromine
HBr
34
Briefly describe 3 of the 5 oxidation rules.
The second rule is the ion chare rule. This rule states that the oxidation number of an element is formed by its charge. For example, halogens main charge is -1 because they only need to gain one electron to be happy, so it is -1 when it is bonded with a normal metal. The third rule is the zero sum rule. This rule states that the oxidation numbers in a compound must come together to form zero. The fourth rule states that there is almost a mini pattern of oxidation numbers. Group 1 elements have the oxidation number of +1. Alkaline earth metals have the oxidation number +2. Oxygens main oxidation number is -2, unless it is bonded with flourine which then it's oxidation number is -1. And halogens, when bonded with a metal have an oxidation number of -1.
35
An expression that represents a chemical reaction by using chemical formulas, chemical symbols, and coefficients
Chemical equation
36
Substances present before a chemical reaction
Reactants
37
Substances present after a chemical reactions
Products
38
Chemical equation that follow the law of mass conservations (equal substances on both sides of the equation)
Balanced equation
39
Tells how many atoms, ions, molecules, or formula units are present in a chemical equation
Coefficients
40
Reactions that occur both forward and in reverse
Reversible reactions
41
Arrangement of metals in order of the activity
Activity series
42
Substances that appear in the reactions and products that remain unchanged
Spectator ions
43
- Identifies all substances involved in a reaction
- Shows the composition of the substances involved
- Indicates the mass of products and reactants
- Accounts for all atoms involved in the reaction
Which of the following does not represent a function of a balanced equation?
Indicates the mass of products and reactants
44
An equation may be balanced by adjusting the coefficients or the subscripts. T/F
False
45
Identify the following reaction that is occurring: 4Fe + 3O2 --> 2Fe2O3
Synthesis is reaction
46
Identify the following reaction that is occurring:
| 2AlCl3 --> 2Al + 3Cl2
Decomposition reaction
47
Identify the following reaction that is occurring:
| 2NaCl + H2SO4 -> Na2SO4 + HCl
Double replacement reaction
48
Identify the following reaction that is occurring:
| TiCl4 + 4Na -> Ti + 4NaCl
Single replacement reaction
49
Identify the following reaction that is occurring:
| Mg(OH)2 + 2HNO3 -> Mg(NO3)2 + 2H2O
Double replacement reaction
50
Identify the following reaction that is occurring:
| NH3 + CO2 + H2O -> NH4HCO3
Synthesis reaction
51
Indicates a gaseous product
(g)
52
Indicates the substance is dissolved in water
(aq)
53
Indicates a solid reaction
(s)
54
Means yield or produces
---->
55
Indicates a liquid reactant or product
(l)
56
The solid that falls out of a solution
Precipitate
57
What is the only thing you are allowed to change when balancing an equation?
Coefficients
58
When looking at an activity series, the higher up an element is, the more reactive it is. T/F
True
59
Formula that shows the type of atoms involved, the exact composition of each molecule, and the arrangement of chemical bonds
Structural formula
60
The mass of one mole of any pure substance
Molar mass
61
Formula that tells what elements are present and give the simplistic whole number ratio of atoms in the compound
Empirical formula
62
The coefficients from the balanced equations give the rations retween the moles of one substance
Mole ratios
63
The ratio of elements in a compound is constant for every particle in that compound
Law of definite composition
64
One mole is equal to avegadro's number. T/F
True
65
What is the mathematical relationship between the amounts of reactants and products in a chemical reaction?
Stoichiometry
66
What is used up before the other reactants?
Limiting reactants
67
What is the measured around of products at thee d of a reaction?
Actual yield
68
What is the maximum amount of products that could be created from a given amount of reactants?
Theoretical yield
69
The number of helium is equal to the number of lead atoms Ina mole of lead. T/F
True
70
Shows the type and numbers of atoms involved as they appear in the molecule
Molecular formula
71
A mole of sucrose has the same mass as a mole of water molecules. T/F
False
72
A molecular compound may have identical empirical and molecular formulas. T/F
True
73
The mole must be used to quantify both large objects as well small objects. T/F
False
74
Conversions from gram to moles
amu
75
Conversion from mole to mole
Molar ratio
76
Conversion from moles to number of particles
Avegadro's number
77
A gas easily mingles with another porous substance
Permeability
78
High pressure can squeeze into smaller volumes
Compressibility
79
A gas moves through a tiny opening into an evacuated chamber
Effusion
80
Collisions of gas molecules conserve energy
Elasticity
81
A gas quickly expands to fill a low pressure region
Expansibility
82
Gas molecules move constantly to uniformly fill their container
Diffusion
83
Diffusion could not occur if molecules were not in constant motion. T/F
True
84
- gas particles move randomly and rapidly
- gas particles lose energy when they collie with one another
- gas particles are separated by great distances
- gas particles do not interact with each other except during momentary collisions
Which one is not a prediction of the kinetic- molecular theory?
Gas particles lose energy when they collide with one another
85
Which gas law focuses on the relationship between pressure and volume?
Boyles law
86
Which property of gases best explains why spooked meat in a sealed plastic container eventually makes a refrigerator smell?
Permeability
87
Gases temperatures must be measured in Celsius temperatures. T/F
False
88
The gas law that focuses on the relationship between volume and temperature is
Charles law
89
If you are collecting gas by water displacement, you must Renee to adjust for
Vapor pressure
90
Collisions constantly change the speed and direction of gas molecules. T/F
True
91
What pair is related by an inverse relationship?
Volume and pressure
92
All gas molecules of the same type have the same speed at the same temperature. T/F
False
93
The SI unit for pressure is the pascal. T/F
True
94
The abbreviation STP represents the standard condition of 760 ATM and 273 K. T/F
False
95
Depends on the force and number of collisions per second
Pressure
96
Determined on the average kinetic energy of molecules
Temperature
