Chemistry Final 24-25 Flashcards
(118 cards)
1
Q
The thing that is fully consumed first in a chemical reaction
A
The Limiting Reactant
2
Q
How many electrons are in the outermost principle energy level of sodium
A
1 Electron
3
Q
how many valence electrons do alkali metals contain
A
1 Electron
4
Q
how many valence electrons do the Halogens (Group 7) contain
A
7 electrons
5
Q
The __________ point is the same temp as the __________ point
A
Freezing and Melting
6
Q
Phase changes are _________ changes
A
Physical
7
Q
__________ have indefinite shapes and indefinite volumes
A
Gasses
8
Q
___________ have indefinite shapes and definite volumes
A
Liquids
9
Q
_________ have definite shapes and definite volumes
A
Solids
10
Q
___________ properties describe how a substance interacts with other substances
A
Chemical
11
Q
____________ properties can be observed without chemically changing matter
A
Physical
12
Q
Physical Changes are?
A
Boiling Point, Tearing Paper, Ductility, Texture, Density, and Evaporation
13
Q
Chemical Changes are?
A
Combustibility, Flammability, Tendency to Corrode, Digestion of Food, Fireworks Exploding, and A Candle Burning
14
Q
There are ____ elements discovered
A
118
15
Q
Elements _____ are Naturally Occuring
A
1-92
16
Q
The lightest element is ___________
A
H (Hydrogen)
17
Q
____________ can be both Anions and Cations
A
Metalloids
18
Q
_________ are Anions
A
NonMetals
19
Q
_______ are Cations
A
Metals
20
Q
Ion means?
A
An Atom With a Charge or Protons are Not Equal to Electrons
21
Q
The atoms in Ions are?
A
Neutral
22
Q
Who identified 11 new elements, all of them greater than 92?
A
Glenn Seaborg
23
Q
The modern periodic table was made by ___________________, he listed everything by the number of protons AKA the atomic number
A
Henry Moseley
24
Q
Who was the father of the periodic table?
A
Dimitri Ivanovich Mendelev or just Mendelev
25
What is on the bottom of the periodic table?
The Actinides
26
What is right above the Actinides?
The Lanthanides
27
What two groups are placed below the Periodic table?
The Lanthanoids and Actinoids
28
Group 17 are the what?
Halogens
29
Group 18 are the what?
Noble gasses
30
Group 2 are the what?
The Alkaline Earth Metals
31
Group 1, except H (Hydrogen) are the what?
The Alkali Metals
32
There are how many columns (Groups or Families) on the periodic table?
18
33
A type 2 binary molecule is a?
Metal + Nonmetal
34
A type 1 binary molecule is a?
Metal + Metalloid
35
You should always assume covalents are what unless told otherwise?
Liquids
36
Ionics are what because they have Tight Geometric Arrangements?
Solids
37
All Metalloids are what?
Solids
38
The two liquid metals are what?
Hg (Mercury) and Br (Bromine)
39
All gasses are either what or what?
Diatomic or Noble
40
All metals except Hg (Mercury) and Br (Bromine) are what?
Solid
41
C (Combustion) means what?
O2 is One of The Reactants (Anything+O2=Anything)
42
DR or DD (Double Replacement or Displacement) means what?
Two Ionic Compounds Trade Partners, Usually as (aq) (AC+BD=AD+BC)
43
SR or SD (Single Replacement or Displacement) means what?
One Free Element Replaces a Less Active Element in a Compound (A+BC=B+AC)
44
D (Decomposition) means what?
One Substance Breaks Down Into Two or More Simpler Substances (AB=A+B)
45
S (Synthesis) means what?
Two or More Substances Combine to Make One Substance (A+B=AB)
46
(aq) means what?
Aqueous
47
(l) means what?
Liquid
48
(s) means what?
Solid
49
(g) means what?
Gas
50
Ate turns to what?
Ic
51
Ite turns to what?
Ous
52
Hypo+Ide turns to what?
Hydro+Ic
53
Acids start there formulas with what?
H
54
In a polyatomic molecule you use ________________________ and list the ___________
The Binary Rules and Charges
55
You do not list the ____________ and you do use ____________ in a Type 3 Covalent Molecule
Charges and Prefixes
56
You list the ___________ and use _____________________ in a Type 2 Ionic Molecule
Charges and Roman Numerals
57
You list the what in a Type 1 Ionic Molecule?
Charges
58
Polyatomic molecules contain what?
3 or More Metal Elements
59
Type 2 Ionic is a metal+a nonmetal from all groups except what?
1, 2, and Al (Aluminum)
60
Type 1 Ionic is a metal+a nonmetal from what groups?
1, 2, and Al (Aluminum)
61
What combine in covalent bonds?
Two NonMetals
62
Everything gets a prefix except the first element if it has a coefficient of what?
1
63
The second element in a covalent bond changes the end of their name to what?
Ide
64
Type 3 binary molecules are __________________ and are _____________
Covalent Bonds and Not Ionic
65
Dec or Deca means what?
10
66
Nona means what?
9
67
Octa means what?
8
68
Hepta means what?
7
69
Hexa means what?
6
70
Penta means what?
5
71
Tetra means what?
4
72
Tri means what?
3
73
Di means what?
2
74
Mono means what?
1
75
Two nonmetals combine in what?
Covalent Bonds
76
1mL of water is equal to what?
1 Gram
77
1 Gram of water is equal to what?
1 mL
78
Stoichiometry is what?
The Process of Using a Chemical Equation to Calculate The Relative Masses of Products and Reactants Involved in a Reaction
79
The Mole Ratio is the what?
Conversion Factors
80
The formula for Percent Yield is what?
Percent Yield=The Actual Yield Divided by The Theoretical Yield Multiplied by 100 (P=A/T*100)
81
What is the quantitative description of the concentration of a solution?
Molarity
82
The equation for M2 is what?
Volume-1 Multiplied by Molarity-1=Molarity-2 Divided by Volume-1+Volume-2 (V1*M1=M2/(V1+V2))
83
The equation for V2 is what?
Volume-1 Divided by Molarity-1=Volume-2 Multiplied by Molarity-2 (V1/M1=V2*M2)
84
M1*V1=Moles=?
M2*V2
85
The equation for Volume is what?
V=Moles Divided by Molarity (V=m/M)
86
The equation for Moles is what?
m=Molarity Multiplied by Volume (m=M*V)
87
The equation for Molarity is what?
M=Moles Divided by Volume (M=m/V)
88
When a solvent has dissolved all the solute it can at a particular temperature, it is said to be what?
Saturated
89
This term is used by chemists to quantitatively describe a solution in which a relatively small amount of solute is dissolved, what is this term?
Dilute
90
In soda, CO2(g) is a ________ and water is the ________
Solute and Solvent
91
There is how many lone pair of electrons in the Lewis structure for Ammonia, NH3?
1
92
When the Alkali Metals react chemically they what?
Lose 1 Electron
93
One of the most important qualities of the water molecule is its _________, which allows it to surround and attract both positive and negative ions
Polarity
94
If an atom forms a diatomic molecule with itself, the bond is what?
Nonpolar Covalent
95
The most electronegative element is what?
F (Fluorine)
96
Chemical bonds formed by the attraction of oppositely charged Ions are called what?
Ionic Bonds
97
When electrons are shared unequally, chemists call these types of bonds what?
Polar Covalent
98
What generally increases as you move from the lower left to the upper right on the periodic table?
The Ionization Energy
99
Metal atoms tend to ______ electrons and form ________ ions, these are also known as (________)
Lose, Positive, and Cations
100
What element has the highest ionization rate?
He (Helium)
101
When moving down a group (family) in the periodic table, the number of valence electrons what?
Remain Constant
102
The Alkali Metals have how many Valence Electrons?
1
103
What is Empirical Formula?
A formula giving the proportions of the elements present in a compound but not the actual numbers or arrangement of atoms.
104
What is Mass Percent?
A way to express the concentration of a component in a solution or mixture by comparing its mass to the total mass of the mixture, expressed as a percentage.
105
What is Molar Mass?
The mass of one mole of a substance.
106
What is Molecular Formula?
A chemical formula that represents the actual number of atoms of each element in a molecule.
107
What is a Mole?
The SI unit for amount of substance.
108
What is a Chemical Reaction?
A process where one or more substances (reactants) are transformed into new substances (products) with different chemical properties.
109
What is a Product?
The substance created in a Chemical reaction.
110
What Is a Reactant?
A substance that takes part in and undergoes change during a reaction.
111
What is a Coefficent?
The number that goes in front of an element in a Chemical formula.
112
What is an Electrolyte?
A substance that, when dissolved in a solvent (typically water), produces a solution that can conduct electricity.
113
What is a Non-Electrolyte?
A substance that does not dissociate into ions when dissolved in a solvent.
114
What is an Excess Reactant?
The Reactant that is left over after a chemical reaction, AKA not the Limiting reaction, the opposite.
115
What is an Actual Yield?
The amount of product created in a chemical reaction.
116
What is a Theoretical Yield?
The calculated amount of product that will be created in a chemical reaction.
117
What does Un-Saturated mean?
A solution that has not reached its maximum solubility and can dissolve more solute.
118
What does Concentrated mean?
That a solution has a relatively large amount of dissolved solute.
