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Jahrdenas_GEAS > Chemistry > Flashcards

Chemistry Flashcards

1
Q

mixture separation technique that separates solids from liquid

A

decantation

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2
Q

mixture separation technique that allows to pass through porous medium

A

filtration

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3
Q

mixture separation technique that vaporizes liquid and condenses it

A

distillation

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4
Q

distillation technique that utilizes narrow difference in boiling point

A

fractional distillation

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5
Q

distillation technique that utilizes separation of volatile oils from plants

A

steam distillation

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6
Q

mixture separation technique that uses tools like foreceps, sieves and etc

A

mechanical separation

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7
Q

mixture separation technique that uses centrifuge

A

centrifugation

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8
Q

mixture separation technique that allows substance to be absorb on surface of inert substance

A

chromatography

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9
Q

mixture separation technique that utilizes difference in solubility

A

solvent extraction

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10
Q

mixture separation technique that extracts gold from ore

A

amalgation

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11
Q

mixture separation technique that extracts gold from ore using cyanide

A

cyanidation

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12
Q

what are the seven SI units

A 
Mass (kg)
Length (m)
Time (s)
Temp (K)
Electric current (A)
Amount of substance (mole)
Luminous Intensity (candela)
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13
Q

when was SI units established? the governing body that facilitates that SI systems?

A

1960, general conference of weighs and measures

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14
Q

the kilogram and meter standard measurement is based on what object?

A

platinum iridium object

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15
Q

Radius of Earth

A

6.371 x 10^6 m

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16
Q

distance of 1 light year in meter

A

9.46 x 10^15 m

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17
Q

Radius of Moon

A

1.74 x 10^6 m

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18
Q

length of one astronomical unit

A

1.5 x 10^11 m

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19
Q

one astronomical unit represent what distance?

A

earth to sun

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20
Q

distance of earth to moon

A

3.84 x 10^8 m

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21
Q

Mass of Earth

A

5.972 x 10^24 kg

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22
Q

Mass of Sun

A

2 x 10^30 kg

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23
Q

Mass of Universe

A

10^50 kg

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24
Q

Mass of Moon

A

7.35 x 10^22 kg

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25
Q

1 pound in kg

A

0.454 kg

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26
Q

density of water

A

1 x 10^3 kg/m^3

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27
Q

density of air

A

1.29 x 10^3 kg/m^3

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28
Q

mass of proton is __________ x mass of electron

A

1836

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29
Q

mass of neutron is __________ x mass of electron

A

1839

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30
Q

volume of nucleus is __________ x volume of atom

A

1/1013

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31
Q

diameter of nucleus

A

1 x 10^-14 m

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32
Q

diameter of nucleus is ________ x diameter of atom

A

1/100,000

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33
Q

Important electron facts

A

JJ thompson
-1.6 x 10^-19 coloumb
1897

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34
Q

Important proton facts

A

Ernest Rutherford
1.6 x 10^-19 coloumb
1911

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35
Q

Important neutron facts

A

James Chadwick
0 coloumb
1932

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36
Q

energy of electron

A

h x freq (in Joules)

h = 6.626 x 10^-34 (J.s) (Plank’s constant)

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37
Q

1 eV in joules

A

1.6 x 10^-19 Joules

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38
Q

momentum of electron

A

h / freq

h = 6.626 x 10^-34 (J.s) (Plank’s constant)

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39
Q

Boltzman’s constant

A

k = 1.38 x 10^-23 (J/K)

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40
Q

Formula for number of electrons per shell

A

2 x n^2

n = energy level

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41
Q

Maximum number of electrons in a subshell

A 
2 x (2L+1)
L= s(0), p(1), d(2), f(3)
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42
Q

The four quantum numbers

A

Principal (n)
Azimutal (L)
Magnetic (M)
Spin (S)

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43
Q

Principal quantum number depicts?

A

energy level (n)

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44
Q

Azimutal quantum number depicts?

A

Magnitude of angular momentum (L)
determines shape
0-s 1-p 2-d 3-f
from 0 to n-1

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45
Q

Magnetic quantum number depicts?

A 
orientation (M)
defines direction of angular momentum
s = 0
p = -1,0,1
d = -2,-1,0,1,2
f = -3,-2, -1, 0, 1, 2, 3
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46
Q

Spin quantum number depicts?

A

Spin (S)

either positive 1/2 or negative 1/2

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47
Q

Another term for either a proton or a neutron?

A

Nucleon

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48
Q

Another term for Electron

A

Negatron

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49
Q

Another term for Hydrogen - 2 Isotope

A

Deuterium

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50
Q

Nucleus of Deuterium

A

Deutereon

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51
Q

Alpha particle Consists of?

A

Nucleus of Helium (+2 Charge)

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52
Q

Beta Particle consists of?

A

electron

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53
Q

What is a Neutrino

A
  • Zero Mass
  • Moves @ the speed of light
  • coems from a Beta Particle Decay
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54
Q

1st Antimatter Particle Discovered?

A

Positron

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55
Q

What is a Positron?

A

a “positive electron”

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56
Q

Another term for Hydrogen - 3 Isotope

A

Tritium

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57
Q

Building blocks of protons and neutrons

A

Quarks

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58
Q

Protons are made up of what quarks?

A

TWO up quarks, ONE down quark

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59
Q

Neutrons are made up of what quarks?

A

TWO down quarks, ONE up quark

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60
Q

Charge of an up quark?

A

+2/3

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61
Q

Charge of a down quark?

A

-1/3

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62
Q

s, p, d, and f are short for?

A

Sharp, Principal, Diffuse, Fundamental

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63
Q

Who discovered quarks? and when?

A

Murray Gell-Mann, 1968

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64
Q

Number that describes the identity of the element?

A

Atomic no.

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65
Q

atomic number is equivalent to the number of ____________ in a non-ion element?

A

protons and electrons

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66
Q

Mass number is equivalent to?

A

protons + # neutrons

   OR

Atomic# + #neutrons

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67
Q

Representative Elements?

A 
1A - Alkali Metals
2A - Alkaline Earth Metals
3A - Boron Group
4A - Carbon Group
5A - Nitrogen Group
6A - Chalcogens
7A - Halogens
8A - Noble/Rare Gases
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68
Q

in the The Group Designation of Representative elements (ex. 1A, 2A, etc.), what do the numbers represent?

A

the number of valence electrons

EXCEPT HELIUM

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69
Q

How many electrons do transition metals have in their shells?

A

More than 8 electrons

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70
Q

What shells in a transition metal is used for bonding w/ other elements??

A

the two outermost shells

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71
Q

What groups do transition metals belong to?

A

1B - 7B

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72
Q

Elements with full outermost shells

A

Noble gases

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73
Q

Are noble gases monoatomic or diatomic?

A

Monoatomic

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74
Q

the 6 noble gases

A 
Helium(2)
Neon(10)
Argon(18)
Krypton(36)
Xenon(54)
Radon(86)
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75
Q

Atomic Number of all Lanthanides? And how many are there?

A

57 - 71

15 total

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76
Q

Other Lanthanide Properties

A
  • AKA rare earth metals/Inner transition metals
  • Naturally found in nature
  • One of the elements are radioactive
77
Q

Atomic Number of all Actinides? And how many are there?

A

89 - 103

15 total

78
Q

Other Actinide Properties

A
  • Synthetic

- Mostly Radioactive

79
Q

What century are the elements arranged by atomic mass?

A

early 19th century

80
Q

the law that states that every 8th element have the same properties?

A

Law of Octaves

81
Q

Who proposed the Law of Octaves? And When?

A

John Newlands, 1864

82
Q

Who proposed the Modern Periodic table? and When?

A

Dmitri Mendeleev & Lothar Meyer, 1869

83
Q

How many elements did the modern periodic table have in 1869?

A

66 elements

84
Q

Who stated that the atomic number is proportional to the atomic mass? and when?

A

Henry Mosely

85
Q

What property in the periodic table increases from lower left to upper right?

A

Non-Metallic Character
Electron Affinity
Ionization Energy

86
Q

What property in the periodic table increases from upper right to lower left?

A

Atomic Radius

Metallic Characteristic

87
Q

Ability of atom to gain or lose electron

A

Metallic Characteristic

88
Q

Energy produced when neutral atom gains an electron to become a negative ion

A

Electron Affinity

89
Q

Energy required to remove electron from element to produce cation

A

Ionization Energy

90
Q

Atomic number and molar mass of Hydrogen, Helium and Lithium

A 
Hydrogen = 1,1
Helium = 2, 4
Lithium = 3, 6.94
91
Q

Atomic number and molar mass of Boron, Carbon and Nitrogen

A 
Boron = 5, 10.8
Carbon = 6, 12
Nitrogen = 7, 14
92
Q

Atomic number and molar mass of Oxygen, Flourine and Sodium

A 
Oxygen = 8, 16
Flourine = 9, 19
Sodium = 11, 23
93
Q

Atomic number and molar mass of Aluminum, Silicon and Phosphorous

A 
Aluminum = 13, 27
Silicon = 14, 28
Phosphorous = 15, 31
94
Q

Atomic number and molar mass of Sulfur, Chlorine and Potassium

A 
Sulfur = 16, 32
Chlorine = 17, 35.5
Potassium = 19, 39
95
Q

Atomic number and molar mass of Titanium, Iron, Nickel and Copper

A 
Titanium = 22, 47.87
Iron = 26, 55.85
Nickel = 28, 58.7 
Copper = 29, 63.55
96
Q

What is a good estimate for molar mass of any element?

A

twice of the atomic number

97
Q

Diatomic Gases

A

H2, O2, N2, F2, Br2, Cl2, I2 , Air

Have No Fear Of Ice Cold Beer

98
Q

What law states that “every distinct compound has its own definite ratio of masses of its component element”

A

Law of Definite Proportions

99
Q

Define as the different forms of one element

A

Allotropes

100
Q

Charge of an anion and cation

A 
Anion = negative
Cation = positive
101
Q

Chemical formula that shows exact ratio of elements in a compound

A

Molecular Formula

102
Q

Chemical formula that shows simplest relative ratio of elements in a compound

A

Empirical Formula

103
Q

How to solve empirical formula?

A

assume 100g of solution

104
Q

Avogadro’s number

A

in 1 mol = 6.022 x 10^23 particles

105
Q

Mass per one mole substance

A

molar mass

1 u = 1 amu = 1 dalton = 1 g/mol = 1.66 x 10^-27 kg

106
Q

Occurs when nucleus breaks down into smaller particles

A

Radioactivity

107
Q

Positively charged particles, with the LOWEST energy level that comes from radioactive decay

A

Alpha Particle

108
Q

Negatively charged particles, that comes from radioactive decay

A

Beta Particle

109
Q

Neutrally charged particles, with the HIGHEST energy level that comes from radioactive decay

A

Gamma Particle

110
Q

nuclear reaction that results from two nuclei combining

A

Fusion

111
Q

nuclear reaction that results from the splitting of the nucleus

A

Fission

112
Q

Quantitative Analysis between reactants and products

A

Stoichiometry

113
Q

The compound in a chemical reaction that runs out first

A

Limiting Reactant

114
Q

The compound that leaves a remainder or residue of that same compound

A

Excess reagent

115
Q

Gas Law relating Pressure and Temperature

A

Gay-Lussac’s Law

116
Q

Gas Law Relating Pressure and Volume

A

Boyles Law

117
Q

Gas Law Relating Volume and Temperature

A

Charle’s Law

118
Q

Gas law relating Volume and the amount of substance

A

Avogadro’s Law

119
Q

Law that states that the total pressure in a system is a superposition of the pressures contributed by the individual gases

A

Dalton’s Law of Partial Pressures

P(sub T) = P1 + P2 + P3 + …

120
Q

The summation of all Mole fractions for a given compound

A

1

121
Q

the mole fraction is obtained by:

A

(#moles of element) / (summation of all #moles of all elements in a compound) :
(n / (n1 + n2+ n3 +…))

                    OR

(partial Pressure of element in inquiry) / (Summation of all partial pressures, or total pressure) :
(Pn / (P1 +P2+P3+…))

122
Q

The Law that states that the the rate of diffusion/effusion of a particle is inversely proportional to the square root of its molar mass

A

Graham’s Law of Diffusion

123
Q

Formula for Graham’s Law of Diffusion

A

( Ra / Rb ) = sqrt( MMb / MMa)

124
Q

The Difference of diffusion from effusion

A

Diffusion - Spread out in open space

Effusion - Escape from membrane/hole

125
Q

Ideal Gas Law

A

PV = nRT

126
Q

what is ‘R’ when using liters for volume and atm for pressure?

A

0.0821 ((L . atm)/(mol . K))

127
Q

what is ‘R’ when using m^3 for volume and Pascal for pressure?

A

8.314 ( Joules / (mol . K) )

128
Q

What is Pressure in CGS

A

dynes/cm^2

129
Q

Formula for Kinetic Energy (in terms of mass and velocity)

A

KE = 0.5 m V^2

130
Q

‘V’ is the velocity in the formula for Kinetic energy and is defined as?

A

Brownian Movement - seemingly random particle movement

131
Q

Formula for Kinetic Energy (in terms of Temperature)

A

KE = 1.5 K T

K - Boltzmann’s Constant (1.38 x 10^23)

132
Q

It is the most probable speed of a molecule based on the Maxwell-Boltzmann Distribution

A

Vrms in Kinetic Theory of Gasses

133
Q

Vrms formula in Kinetic Theory of Gasses

A

Vrms=sqrt((3KT)/m)
K=boltzmann constant
T=Temperature in Kelvin
m=mass of the particle

134
Q

Type of bonding due to the electrostatic attraction of ions

A

Ionic Bond

135
Q

Bonding that occur due to the sharing of electrons

A

Covalent Bond

136
Q

Maximizes 8 valence electron when covalent bonding occurs (Except with hydrogen(only 2 VE))

A

Octet Rule

137
Q

Ability of atoms to attract electrons towards itself

A

Electronegativity

138
Q

Electronegativity was first recorded by?

A

Linus Pauling

139
Q

described as when electrons spend more time near the vicinity of one atom

A

Polar Bonding

140
Q

Process of electrically polarizing a material

A

Induction

141
Q

The four Intermolecular forces

A

Dipole-Dipole
Ion-Dipole
London Dispersion
Hydrogen forces

142
Q

Intermolecular force where Negatively polarized portion of one atom is attracted to a positively polarized portion of another atom

A

Dipole-Dipole Force

143
Q

Intermolecular force where a polarized Ion attracts the oppositely charged portion of a polarized atom

A

Ion-Dipole Force

144
Q

Intermolecular force where due to the motion of non-polar molecules, causing temporary dipoles. The force is only significant when atoms are close

A

London Dispersion Force

145
Q

A Dipole-Dipole Force involving Hydrogen

A

Hydrogen Force

146
Q

A solution that has more solvent than solute

A

Homogenous mixture

147
Q

Substances that can never be dissolved after mixing

A

Precipitates

148
Q

Three situations of a solution based on saturation

A

Saturated
Unsaturated
Supersaturatied

149
Q

The solution’s situation wherein solute separates from solvent, forming crystals

A

Supersaturated

150
Q

the description of a solution when the solvent used is water

A

Aqueous

151
Q

Two types of Aqueous solutions

A

Electrolytes - Can facilitate electron flow

Non-electrolytes - cannot facilitate electron flow

152
Q

process of surrounding a solute with a solvent

A

Solvation

153
Q

process of surrounding a solute with a solvent, PARTICULARLY WATER

A

Hydration

154
Q

A figure of merit for concentration that depicts the percentage of mass of a solute compared to the total mass of the solution (and its formula)

A

% By Mass = (Mass Solute / Mass solution) x 100%

155
Q

A figure of merit for concentration that depicts the amount of substance of a solute in comparison to the Volume of a solution in Liters

A

Molarity(M) = (Mol Solute)/(Vol. Solution(in Liters))

156
Q

A figure of merit for concentration that depicts the amount of substance of a solute in comparison to the mass of the solvent in kg

A

Molality(m) = (Mol Solute)/(Kg Solvent(in Kg))

157
Q

Formula used for solving Dilution Problems

A

(Molality1)(Volume1) = (Molality2)(Volume2)

158
Q

It is a Heterogeneous Mixture - a substance dispersed throughout another substance

A

Colloid

159
Q

A colloid that have liquid particles dispersed throughout a liquid

A

Emulsion

160
Q

A colloid that have solid or liquid particles dissolved throughout a gas

A

Aerosol

161
Q

The effect were if light passes through a colloid, the light disperses throughout it

A

Tyndall Effect

162
Q

Who defined the definition of an acid and a base?

A

Svante August Arrhenius

163
Q

Bronsted defines Acids as _____________ and bases as ____________

A

Acids as Proton donors, bases as Proton Acceptors

164
Q

Acid + Base = Water + Salt

what do you call this reaction?

A

Neutralization Reaction

165
Q

What scale measures the power of hydrogen in a substance? and who proposed this scale?

A

pH Scale, Soren Sorensen

166
Q

Formula for pH value

A

pH = -log[H+]

where H+ is the Molarity(M) of the hydrogen Ion with respect to the substance’s Volume in liters

167
Q

Formula for pOH Value

A

pOH = -log[OH-]

where OH- is the Molarity(M) of the Hydroxide Ion with respect to the substance’s Volume in liters

168
Q

The formula that relates the pH and the pOH value

A

pH + pOH = 14

169
Q

Acid Properties

A
  • Sour
  • Blue&raquo_space;> Red Litmus paper
  • Reacts w/ Metals to produce Hydrogen
  • Reacts w/ carbonates to produce CO2
  • Electrically Conductive (aqueous)
  • pH value from 1 to 7 (1 is the highest acidity level, and the lowest basicity level)
170
Q

Base Properties

A
  • Bitter
  • Red&raquo_space;> Blue Litmus paper
  • Slippery
  • Electrically conductive (aqueous)
  • pH value from 7 to 14 (14 is the highest basicity level, and the lowest acidity level)
171
Q

pH value of a neutral substance

A

pH(neutral) = 7

172
Q

The Breakdown of Sugar

A

Glycolysis

173
Q

The building of sugars from light, Oxygen, and water

A

Photosynthesis

174
Q

Two terms synonymous to “Sugar”

A

Sugar = Carbohydrates = Saccharides

175
Q

Saccharide composed of one sugar molecule

A

Monosaccharide (ex. Glucose)

176
Q

Saccharide composed of two sugar molecule

A

Disaccharide (ex. Table Sugar)

177
Q

Saccharide composed of many sugar molecules

A

Polysaccharide (ex. Starch)

178
Q

Material found in Fat, Steroids, and Wax

A

Lipids

179
Q

Made of glycerol connected to different fatty acids

A

Fat

180
Q

Another term for fat

A

Triglycerides

181
Q

two types of triglycerides

A

Saturated and unsaturated

182
Q

Building block of all living things

A

Nucleic Acids

183
Q

DNA stands for?

A

Deoxyribonucleic Acid

184
Q

Fundamental Building block of Nucleic Acids

A

Nucleobase

185
Q

The five primary Nucleobases

A

Uracil, Cytosine, Thymine, Adenine, and Guanine

186
Q

STP Values

A

273 Kelvin, 1 atm,

187
Q

Volume of 1 mole of gas at STP

A

22.4 Liters

188
Q

Principle used to solve for chemical reactions

A

Law of the Conservation of mass

189
Q

GEAS Default Room temperature

A

T(default) = 20 Celcius

Jahrdenas_GEAS (9 decks)

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