Chemistry Flashcards
(132 cards)
1
Q
Smallest subdivision of an element that can take part in a chemical reaction
A
Atom
2
Q
Smallest subdivision of an element or a compound that can exist in a free state
A
Molecule
3
Q
Electrons in the outermost orbit
A
Valence Electrons
4
Q
Approximately equal to the sum of the number of neutrons and protons in the nucleus
A
Atomic mass
5
Q
Equal to the weighted average of all the masses of the isotopes
A
Atomic mass
6
Q
Equal to the number of protons in the nucleus
A
Atomic Number
7
Q
What orbital is the most stable state that an electron can occupy
A
S orbital
8
Q
As you move from left to right the Atomic Weight ________.
A
Increases
9
Q
The Vertical columns in a periodic table are called?
A
Groups/Families
10
Q
How many total groups/families in the periodic table?
A
18 columns
11
Q
How many columns are in the main groups of the periodic table?
A
8 columns
12
Q
How many columns in the transition metal groups?
A
10 columns
13
Q
How many periods are there in the periodic table?
A
Seven (7)
14
Q
It is the tendency to absorb electrons from neighboring atoms.
A
Electronegativity
15
Q
Negatively charged ions.
A
Anions
16
Q
These are types of ions that lose its electrons at the anode during electro-chemical reaction.
A
Anions
17
Q
An anion becomes negatively charged because it _________ an electron. (Hint: absorb, release)
A
Absorbs
18
Q
In order to become neutral, an Anion must ________ electron.
A
release
19
Q
What do you call the loss of an electron in an ion?
A
Oxidation
20
Q
The charge/no. of electrons absorbed by an ion from neighboring atoms.
A
Oxidation number
21
Q
This refers to the number of electrons that must be lost to achieve charge neutrality.
A
Oxidation number.
22
Q
When an atom loses an electron it becomes ________ charged.
A
Positive
23
Q
These are the positively charged ions
A
Cations
24
Q
These ions gains electrons and are formed at the cathode in electro-chemical reaction.
A
Cations
25
Cations must _______ electrons to become neutral
Gain
26
This refers to the gaining of an electron by an atom/ion
Reduction
27
Also called Electrovalent Bonding
Ionic Bonding
28
The type of linkage or bonding formed from the electrostatic attraction between oppositely charged ions
Ionic Bonding
29
This type of bonding is formed between atoms of high electron affinities and low ionization energies.
Ionic bonding
30
This refers to sharing of electrons
Covalent Bonding
31
The type of bonding common in gases that form diatomic molecules in their free state.
Covalent bonding
32
This type of bonding occurs in elements with same electron affinity and ionization energy.
Covalent Bonding
33
This type of bond is typical in organic compounds
Covalent Bonding
34
Simplest type of Chemical reaction where two elements or compounds combine directly to form a new one.
Direct Combination / Synthesis
35
Another name for the Direct Combination chemical reaction.
Synthesis
36
In this type of Chemical reaction, the bonds uniting a compound are disrupted by heat or another energy source to yield simpler compounds or elements.
Decomposition
37
This type of Chemical reaction is identified by one element and one compound as the reactants
Single Displacement
38
This type of chemical reaction is characterized by having two compounds as reactants and forming two new compounds
Double displacement
39
This type of reaction involves oxidation of one substance and the reduction of another.
Oxidation - Reduction
40
Study of proportions in which elements combine into compounds
Stoichiometry
41
This refers to the no. of gram equivalent weights of solute per liter of solution
Normality
42
Refers to the no. of grams mole per liter of solution
Molarity
43
Refers to the gram formula weights per liter of solution
Formality
44
Refers to the no. of gram moles of solute per 1000 grams of solvent.
Molality
45
Refers to the no. of moles of solute divided by the no. of moles of solvent and all solutes
X mole fraction
46
These are any substance/s that dissociates in water into H+ or H3O+
Acids
47
These substances dissociates in water and gives up OH-
Bases
48
Charge in an electron
- 1.6 x 10^-19 C
49
Charge in a proton.
+1.6 x 10^-19 C
50
Weight of an electron
9.109 x 10^-31 kg
51
1 amu = ________ kg
1.67 x 10^-27 kg
52
1 amu = ______ g/mol
1 g/mol
53
It is equal to the number of molecules per element in a compound multiplied with amu.
Molecular Mass/Weight
54
1 mole = _______ atoms/molecules
Avogadro's Number (6.02 x 10^23 atoms/molecules)
55
Formula for percent composition of an element in a compound.
MW(element) / Sum of the total MW in the compound
56
In Ideal Gas Laws, the value of R to be used when you are given
L-atm/mol-K
0.0821
57
In Ideal Gas Laws, the value of R to be used when you are given
J/mol-K
8.314
58
Ideal Gas law variant where the Temperature is held constant.
Boyle's Law
59
Formula for Boyle's Law
P1V1 = P2V2
60
Ideal Gas Law variant where the Pressure is held constant.
Charles' Law
61
Formula for Charles' Law
V1/V2 = T1/T2
62
Ideal Gas Law variant where the Volume is held constant
Gay-Lussac's Law
63
Formula for Gay-Lussac's Law
P1/P2 = T1/T2
64
It states that the total pressure is equal to the sum of the individual Pressure of all the gases in a container.
Dalton's Law of Pressure
65
Ideal Gas Law Variant where the Pressure and Temperature are held constant
Avogadro's Law
66
Formula for Avogadro's Law
V1/V2 = n1/n2
67
Formula for Ideal Gas Law
PV = nRT
68
Formula for Combined Gas Law
(P1V1)/(P2V2) = T1/T2
69
The mass of the proton with respect to the mass of the electron
Mp = 1836 Me-
70
The mass of the neutron with respect to the mass of the electron.
Mn = 1839 Me-
71
This refers to variants of an atom with same no. of protons but with different neutrons
Isotopes
72
Atoms with less than 4 valence electrons are _______?
Conductive
73
Atoms with 4 valence electrons are _________.
Semi-conductive
74
Atoms with more than 4 valence electrons are _______.
Insulating
75
As you move from Right to left, the Atomic Radius _______.
Increases
76
As you move from Top to Bottom, the Atomic Radius _________.
Increases
77
As you move from Left to Right, the Atomic Radius _________
Decreases
78
As you move from Bottom to the Top, the Atomic Radius ________
Decreases
79
As you move from Left to Right , the Ionization Energy _______
Increases
80
As you move from Bottom to Top, the Ionization Energy ________
Increases
81
As you move from Right to Left, the Ionization Energy ________
Decreases
82
What are the 7 Base SI units
m, kg, s, K, A, cd, mol
83
What are the 7 Diatomic Elements
H, N, F, O, I, Cl, Br
| Have No Fear Of Ice Cold Beer
84
Value of the Standard Temperature
273 K
85
Value of the Standard Pressure
1 atm
86
It is the movement of gases from High Concentration to Low Concentration.
Diffusion
87
Formula for Rate of Diffusion.
Rate of Diffusion = (amount of gas passing an area) / (unit of time)
88
Movement of gas through a small opening
Effusion
89
The Volume of 1 mole of any kind of gas is?e
22.4 Liters
90
Elements in the Group 1A are called?
Alkali Metals
91
Elements in the Group 2A are called?
Alkaline Earth Metals
92
What are the 7 Metalloid Elements?
B, Si, Ge, As, Sb, Te, Po
93
What is the Atomic mass of Helium?
4
94
What is Atomic Mass of Lithium?
7
95
What is the atomic number and mass of Boron?
5, 10.8
96
What is the atomic mass of Carbon?
12
97
What is the atomic mass of Nitrogen?
14
98
What is the atomic mass of Oxygen?
16
99
What is the atomic mass of Fluorine?
19
100
What is the Atomic mass of Na?
23
101
What is the Atomic mass of Mg?
24.3
102
What is the Atomic Mass of Aluminum?
27
103
What is the atomic Mass of Si?
28
104
What is the atomic mass of P?
31
105
What is the atomic mass of Sulfur?
32
106
What is the atomic mass of Chlorine?
35.45
107
What is the atomic mass of K?
39
108
What is the atomic mass of Calcium?
40
109
What is the atomic mass of Chromium?
52
110
What is the atomic mass of Mn?
55
111
What is the atomic mass of Fe?
55.85
112
What is the atomic mass of Ni?
58.7
113
What is the atomic mass of Cu?
63.55
114
What is the atomic mass of Zn?
65.39
115
What is the atomic mass of Br?
80
116
What is the atomic mass of Ag?
108
117
What is the atomic mass of Iodine?
127
118
What is the atomic mass of Gold?
197
119
What is the atomic mass of Hg?
200.5
120
What is the atomic mass of Pb?
207.2
121
The Lanthanides and Actinide Series are also called what?
Inner Transition Metals
122
“When two or more elements form more than one compound, the ratio of the masses of one element that combine with a given mass of another element in the different compounds is the ratio of small
whole numbers.” This statement is known as:
Law of Multiple Proportion
123
This states that the rate of effusion of gas is inversely proportional to the square root of its molecular mass.
Graham's Law
124
“The total pressure of a mixture of gases equals the sum of the partial pressures of each of the gases in the mixture”. This statement is known as __________.
Dalton's Law of Partial Pressure
125
"At a constant temperature, the amount of a given gas that dissolves in a given type and volume of liquid is directly proportional to the partial pressure of that gas in equilibrium with that liquid." An equivalent way of stating the law is that the solubility of a gas in a liquid is directly proportional to the partial pressure of the gas above the liquid: This statement comes from_________?
Henry's Law
126
__________ states that the lowest energy electron configuration, the ground state, in any electron subshell is the one with the greatest number of parallel electron spins.
Hund's Rule
127
In the ____________ of acid-base reactions, bases donate pairs of electrons and acids accept pairs of electrons.
Lewis Theory
128
__________ states that the vapor pressure of a solvent above a solution is equal to the vapor pressure of the pure solvent at the same temperature scaled by the mole fraction of the solvent present:
Raoult's law
129
“When the elements are arranged in the order of increasing atomic number, elements with similar properties appear at periodic
intervals.” This statement is known as _________.
The periodic law
130
This refers to the property of a material that is dependent on the amount of matter present.
Extensive Property
131
This refers to the property of matter that is dependent only on the type of matter present and not on the amount.
Intensive Property
132
It expresses the reaction rate in terms of changes in the concentration of one or more reactants (Δ[R]) over a specific time interval (Δt).
Differential Rate Law
