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ESAS > Chemistry > Flashcards

Chemistry Flashcards

1
Q

Smallest subdivision of an element that can take part in a chemical reaction

A

Atom

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2
Q

Smallest subdivision of an element or a compound that can exist in a free state

A

Molecule

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3
Q

Electrons in the outermost orbit

A

Valence Electrons

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4
Q

Approximately equal to the sum of the number of neutrons and protons in the nucleus

A

Atomic mass

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5
Q

Equal to the weighted average of all the masses of the isotopes

A

Atomic mass

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6
Q

Equal to the number of protons in the nucleus

A

Atomic Number

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7
Q

What orbital is the most stable state that an electron can occupy

A

S orbital

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8
Q

As you move from left to right the Atomic Weight ________.

A

Increases

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9
Q

The Vertical columns in a periodic table are called?

A

Groups/Families

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10
Q

How many total groups/families in the periodic table?

A

18 columns

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11
Q

How many columns are in the main groups of the periodic table?

A

8 columns

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12
Q

How many columns in the transition metal groups?

A

10 columns

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13
Q

How many periods are there in the periodic table?

A

Seven (7)

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14
Q

It is the tendency to absorb electrons from neighboring atoms.

A

Electronegativity

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15
Q

Negatively charged ions.

A

Anions

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16
Q

These are types of ions that lose its electrons at the anode during electro-chemical reaction.

A

Anions

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17
Q

An anion becomes negatively charged because it _________ an electron. (Hint: absorb, release)

A

Absorbs

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18
Q

In order to become neutral, an Anion must ________ electron.

A

release

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19
Q

What do you call the loss of an electron in an ion?

A

Oxidation

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20
Q

The charge/no. of electrons absorbed by an ion from neighboring atoms.

A

Oxidation number

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21
Q

This refers to the number of electrons that must be lost to achieve charge neutrality.

A

Oxidation number.

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22
Q

When an atom loses an electron it becomes ________ charged.

A

Positive

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23
Q

These are the positively charged ions

A

Cations

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24
Q

These ions gains electrons and are formed at the cathode in electro-chemical reaction.

A

Cations

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25
Q

Cations must _______ electrons to become neutral

A

Gain

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26
Q

This refers to the gaining of an electron by an atom/ion

A

Reduction

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27
Q

Also called Electrovalent Bonding

A

Ionic Bonding

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28
Q

The type of linkage or bonding formed from the electrostatic attraction between oppositely charged ions

A

Ionic Bonding

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29
Q

This type of bonding is formed between atoms of high electron affinities and low ionization energies.

A

Ionic bonding

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30
Q

This refers to sharing of electrons

A

Covalent Bonding

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31
Q

The type of bonding common in gases that form diatomic molecules in their free state.

A

Covalent bonding

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32
Q

This type of bonding occurs in elements with same electron affinity and ionization energy.

A

Covalent Bonding

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33
Q

This type of bond is typical in organic compounds

A

Covalent Bonding

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34
Q

Simplest type of Chemical reaction where two elements or compounds combine directly to form a new one.

A

Direct Combination / Synthesis

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35
Q

Another name for the Direct Combination chemical reaction.

A

Synthesis

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36
Q

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.

A

Decomposition

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37
Q

This type of Chemical reaction is identified by one element and one compound as the reactants

A

Single Displacement

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38
Q

This type of chemical reaction is characterized by having two compounds as reactants and forming two new compounds

A

Double displacement

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39
Q

This type of reaction involves oxidation of one substance and the reduction of another.

A

Oxidation - Reduction

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40
Q

Study of proportions in which elements combine into compounds

A

Stoichiometry

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41
Q

This refers to the no. of gram equivalent weights of solute per liter of solution

A

Normality

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42
Q

Refers to the no. of grams mole per liter of solution

A

Molarity

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43
Q

Refers to the gram formula weights per liter of solution

A

Formality

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44
Q

Refers to the no. of gram moles of solute per 1000 grams of solvent.

A

Molality

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45
Q

Refers to the no. of moles of solute divided by the no. of moles of solvent and all solutes

A

X mole fraction

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46
Q

These are any substance/s that dissociates in water into H+ or H3O+

A

Acids

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47
Q

These substances dissociates in water and gives up OH-

A

Bases

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48
Q

Charge in an electron

A
  • 1.6 x 10^-19 C
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49
Q

Charge in a proton.

A

+1.6 x 10^-19 C

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50
Q

Weight of an electron

A

9.109 x 10^-31 kg

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51
Q

1 amu = ________ kg

A

1.67 x 10^-27 kg

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52
Q

1 amu = ______ g/mol

A

1 g/mol

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53
Q

It is equal to the number of molecules per element in a compound multiplied with amu.

A

Molecular Mass/Weight

54
Q

1 mole = _______ atoms/molecules

A

Avogadro’s Number (6.02 x 10^23 atoms/molecules)

55
Q

Formula for percent composition of an element in a compound.

A

MW(element) / Sum of the total MW in the compound

56
Q

In Ideal Gas Laws, the value of R to be used when you are given
L-atm/mol-K

A

0.0821

57
Q

In Ideal Gas Laws, the value of R to be used when you are given
J/mol-K

A

8.314

58
Q

Ideal Gas law variant where the Temperature is held constant.

A

Boyle’s Law

59
Q

Formula for Boyle’s Law

A

P1V1 = P2V2

60
Q

Ideal Gas Law variant where the Pressure is held constant.

A

Charles’ Law

61
Q

Formula for Charles’ Law

A

V1/V2 = T1/T2

62
Q

Ideal Gas Law variant where the Volume is held constant

A

Gay-Lussac’s Law

63
Q

Formula for Gay-Lussac’s Law

A

P1/P2 = T1/T2

64
Q

It states that the total pressure is equal to the sum of the individual Pressure of all the gases in a container.

A

Dalton’s Law of Pressure

65
Q

Ideal Gas Law Variant where the Pressure and Temperature are held constant

A

Avogadro’s Law

66
Q

Formula for Avogadro’s Law

A

V1/V2 = n1/n2

67
Q

Formula for Ideal Gas Law

A

PV = nRT

68
Q

Formula for Combined Gas Law

A

(P1V1)/(P2V2) = T1/T2

69
Q

The mass of the proton with respect to the mass of the electron

A

Mp = 1836 Me-

70
Q

The mass of the neutron with respect to the mass of the electron.

A

Mn = 1839 Me-

71
Q

This refers to variants of an atom with same no. of protons but with different neutrons

A

Isotopes

72
Q

Atoms with less than 4 valence electrons are _______?

A

Conductive

73
Q

Atoms with 4 valence electrons are _________.

A

Semi-conductive

74
Q

Atoms with more than 4 valence electrons are _______.

A

Insulating

75
Q

As you move from Right to left, the Atomic Radius _______.

A

Increases

76
Q

As you move from Top to Bottom, the Atomic Radius _________.

A

Increases

77
Q

As you move from Left to Right, the Atomic Radius _________

A

Decreases

78
Q

As you move from Bottom to the Top, the Atomic Radius ________

A

Decreases

79
Q

As you move from Left to Right , the Ionization Energy _______

A

Increases

80
Q

As you move from Bottom to Top, the Ionization Energy ________

A

Increases

81
Q

As you move from Right to Left, the Ionization Energy ________

A

Decreases

82
Q

What are the 7 Base SI units

A

m, kg, s, K, A, cd, mol

83
Q

What are the 7 Diatomic Elements

A

H, N, F, O, I, Cl, Br

Have No Fear Of Ice Cold Beer

84
Q

Value of the Standard Temperature

A

273 K

85
Q

Value of the Standard Pressure

A

1 atm

86
Q

It is the movement of gases from High Concentration to Low Concentration.

A

Diffusion

87
Q

Formula for Rate of Diffusion.

A

Rate of Diffusion = (amount of gas passing an area) / (unit of time)

88
Q

Movement of gas through a small opening

A

Effusion

89
Q

The Volume of 1 mole of any kind of gas is?e

A

22.4 Liters

90
Q

Elements in the Group 1A are called?

A

Alkali Metals

91
Q

Elements in the Group 2A are called?

A

Alkaline Earth Metals

92
Q

What are the 7 Metalloid Elements?

A

B, Si, Ge, As, Sb, Te, Po

93
Q

What is the Atomic mass of Helium?

A

4

94
Q

What is Atomic Mass of Lithium?

A

7

95
Q

What is the atomic number and mass of Boron?

A

5, 10.8

96
Q

What is the atomic mass of Carbon?

A

12

97
Q

What is the atomic mass of Nitrogen?

A

14

98
Q

What is the atomic mass of Oxygen?

A

16

99
Q

What is the atomic mass of Fluorine?

A

19

100
Q

What is the Atomic mass of Na?

A

23

101
Q

What is the Atomic mass of Mg?

A

24.3

102
Q

What is the Atomic Mass of Aluminum?

A

27

103
Q

What is the atomic Mass of Si?

A

28

104
Q

What is the atomic mass of P?

A

31

105
Q

What is the atomic mass of Sulfur?

A

32

106
Q

What is the atomic mass of Chlorine?

A

35.45

107
Q

What is the atomic mass of K?

A

39

108
Q

What is the atomic mass of Calcium?

A

40

109
Q

What is the atomic mass of Chromium?

A

52

110
Q

What is the atomic mass of Mn?

A

55

111
Q

What is the atomic mass of Fe?

A

55.85

112
Q

What is the atomic mass of Ni?

A

58.7

113
Q

What is the atomic mass of Cu?

A

63.55

114
Q

What is the atomic mass of Zn?

A

65.39

115
Q

What is the atomic mass of Br?

A

80

116
Q

What is the atomic mass of Ag?

A

108

117
Q

What is the atomic mass of Iodine?

A

127

118
Q

What is the atomic mass of Gold?

A

197

119
Q

What is the atomic mass of Hg?

A

200.5

120
Q

What is the atomic mass of Pb?

A

207.2

121
Q

The Lanthanides and Actinide Series are also called what?

A

Inner Transition Metals

122
Q

“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:

A

Law of Multiple Proportion

123
Q

This states that the rate of effusion of gas is inversely proportional to the square root of its molecular mass.

A

Graham’s Law

124
Q

“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 __________.

A

Dalton’s Law of Partial Pressure

125
Q

“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_________?

A

Henry’s Law

126
Q

__________ 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.

A

Hund’s Rule

127
Q

In the ____________ of acid-base reactions, bases donate pairs of electrons and acids accept pairs of electrons.

A

Lewis Theory

128
Q

__________ 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:

A

Raoult’s law

129
Q

“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 _________.

A

The periodic law

130
Q

This refers to the property of a material that is dependent on the amount of matter present.

A

Extensive Property

131
Q

This refers to the property of matter that is dependent only on the type of matter present and not on the amount.

A

Intensive Property

132
Q

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).

A

Differential Rate Law

ESAS (7 decks)

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