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GEAS: General Chemistry > SPLBE 2016 > Flashcards

SPLBE 2016 Flashcards

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1
Q

chemistry is derive from the Arabic word kimia meaning

A

alchemy

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2
Q

is the science that deals with the properties of organic and inorganic substances and their interactions with other organic and inorganic substances

A

chemistry

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3
Q

classification of matter by physical state:

A

solid, liquid, gas, plasma, bose-einstein condensate

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4
Q

rigidly structured materials having a fixed volume and shape

A

solid

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5
Q

has a fixed volume but assumes the shape of its container

A

liquid

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6
Q

most random state of matter, and has no fixed volume and either expands or contracts to fill its container completely

A

gas

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7
Q

is an ionize gas, a gas into which sufficient energy is provided to free electrons from atoms or molecules, to allow, ions and electrons, to exist

A

plasma

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8
Q

is a gaseous superfluid. it occurs at ultra-low temperature (very near to absolute zero), close to the point that the atoms are not moving at all

A

bose condensation

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9
Q

enumerate phase changes:

A

melting, freezing, sublimation, deposition, condensation, evaporation

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10
Q

is the process resulting in change of phase from a solid to a liquid

A

melting

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11
Q

another term for melting

A

fusion

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12
Q

is the phase change from liquid to solid

A

freezing

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13
Q

another term for freezing (phase change)

A

solidification

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14
Q

it is the transition from the solid to gas phase without passing the liquid state

A

sublimation

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15
Q

is a process in which gas transforms into solid

A

deposition

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16
Q

deposition (phase change) is also called as

A

desublimation

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17
Q

is the change in matter of a substance to a denser phase, such as a gas (or vapor) to a liquid

A

condensation

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18
Q

is the conversion of water from a liquid into gas

A

evaporation

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19
Q

two major changes in matter:

A

physical change and chemical change

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20
Q

no change in the basic composition or nature of matter

A

physical change

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21
Q

changing in the basic nature or composition into a new substance or material

A

chemical change

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22
Q

examples of physical change

A

melting, freezing, condensing, breaking, crushing, cutting and bending

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23
Q

examples of chemical change

A

digestion, respiration, photosynthesis, burning, rusting, decomposition….

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24
Q

properties of matter

A

physical and chemical, intensive and extensive

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25
Q

are properties which can be measured without changing the identity and composition of a substance

A

physical properties

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26
Q

examples of physical properties of matter

A

odor, color, density, boiling point, etc….

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27
Q

are properties that lead to changes in the identity and composition of a substance

A

chemical properties

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28
Q

examples of chemical properties

A

combustibility, flammability, toxicity, reactivity, acidity….

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29
Q

are those which do not depend on the size of he sample involved

A

intensive properties

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30
Q

example of intensive properties

A

density, boiling point, freezing point, color, melting point, taste, hardness, reactivity, luster, malleability and conductivity

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31
Q

are those that do depend on the size of the sample involved

A

extensive properties

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32
Q

examples of extensive properties

A

length, width, surface area, volume, mass, and weight

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33
Q

types of matter

A

pure substance, mixture

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34
Q

matter that has a definite composition and boiling point.

A

pure substance

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35
Q

are pure substance which cannot be broken down into simpler substances by ordinary chemical changes

A

elements

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36
Q

composed of two or more elements combined in a fixed proportion.

A

compounds

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37
Q

compounds can be broken down into simpler substances by _____

A

ordinary chemical reactions

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38
Q

elements are represented by

A

symbols

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39
Q

compounds are represented by

A

chemical formula

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40
Q

combination of two or more substances in no fixed proportions which can be separated by physical means

A

mixtures

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41
Q

constituents are not distinguishable even to some extent of magnification

A

homogenous mixture

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42
Q

constituents are readily visible or easily identifiable

A

heterogenous mixture

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43
Q

a collection of matter consisting of a positively charged core and maintains a number of electrons to balance the positive charge in the nucleus

A

atom

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44
Q

positively charged core

A

atomic nucleus

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45
Q

electron mass

A

9.1094E-28 g

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46
Q

electron charge

A

-1.602E-19 C

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47
Q

smallest particle in the atom

A

electron

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48
Q

proton mass

A

1.6726E-24g

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49
Q

proton charge

A

+1.602E-19

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50
Q

proton is _____ times the mass of the electron

A

1,837

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51
Q

neutron mass

A

1.6749E-24g

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52
Q

neutron charge

A

neutral

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53
Q

neutron is ______ times the mass of the electron

A

1,839

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54
Q

to find the maximum no. of electrons per shell:

A

2n^2

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55
Q

smallest known building block of matter

A

quark

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56
Q

up-quarks have electric charges of

A

+2/3

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57
Q

down quarks have charges of

A

-1/3

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58
Q

a proton is made up of

A

two up-quarks and a down-quark

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59
Q

is the smallest indivisible portion of a pure compound that retains a set of unique chemical properties.

A

molecule

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60
Q

consists of two or more atoms bonded together

A

molecule

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61
Q

molecules that contain one atom

A

monoatomic

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62
Q

molecules that contain two atoms

A

diatomic

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63
Q

molecules that contain three atoms

A

triatomic

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64
Q

molecules that contain more than one atom

A

polyatomic

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65
Q

the number of protons in the nucleus

A

atomic number(Z)

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66
Q

is approximately the sum of the number of protons and neutrons in the nucleus of the atom

A

atomic mass number

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67
Q

atomic mass number is the same as the

A

atomic weight(A)

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68
Q

one atomic mass unit is equivalent to

A

1/12 of the mass of an atom of Carbon 12 which is approx. equal to 1.66x10E-27 kg. This was formerly defined as 1/16 of the mass of one atom of oxygen 16

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69
Q

oxygen 16 is also called

A

Dalton, Da

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70
Q

the number of electrons in the outermost shell of an atom

A

valence

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71
Q

they strongly determine the electrical and thermal conductivity of the substance

A

valence

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72
Q

valence electrons that are less than 4 is considered as a

A

conductor

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73
Q

a semiconductor has how many valence electrons

A

4

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74
Q

how many valence electron does an insulator has

A

greater than 4

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75
Q

are formed when atoms gain or lose electrons

A

ions

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76
Q

are formed when a neutral atom loses electrons

A

cations

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77
Q

are formed when a neutral atom gains electrons

A

anions

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78
Q

tend to lose electrons to form positive ions

A

metallic atoms

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79
Q

tend to gain electrons to form negative ions

A

nonmetallic atoms

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80
Q

is an ion which has two negative charges on it

A

dianion

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81
Q

is an ion that contains an odd number of electrons and are mostly very reactive and unstable

A

radical ion

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82
Q

are polyatomic ions containing oxygen, such as carbonate and sulfate

A

oxyanions

83
Q

the charge of an atom or ion is equal to

A

number of protons - number of electrons

84
Q

are elements whose atoms have the same atomic number but different atomic weights.

A

isotopes

85
Q

the nuclei of isotopes differ from one another only in the

A

number of neutrons

86
Q

an isotope that is described as the heavy hydrogen

A

deuterium

87
Q

an isotope of hydrogen that is radioactive

A

tritium

88
Q

is the spontaneous disintegration of atomic nuclei (unstable nuclei) by the emission of radiation particles

A

radioactivity

89
Q

what are the three radiation particles

A

alpha, beta, gamma

90
Q

is a tabular method of displaying the chemical elements.

A

periodic table

91
Q

the periodic table is first devise by

A

Dmitri Mendeleev

92
Q

the periodic table is first devise in the year

A

1869

93
Q

the periodic law states that

A

when the elements are arranged in the order of increasing atomic number, elements with similar properties appear at periodic interval

94
Q

is a vertical column in the periodic table of the elements

A

groups or family

95
Q

are considered the most important way of classifying the elements

A

groups

96
Q

is a horizontal row in the periodic table of the elements

A

periods

97
Q

define noble gases

A

all elements of group 8A have full valence shell. they do not need to react with other elements to attain a full shell, and are therefore unreactive, monoatomic gases

98
Q

is the most inert element among noble gases

A

helium

99
Q

inert means

A

lacking the ability to move

100
Q

Group 8A is also called

A

Group 0 or Group 18 in the new concept

101
Q

define halogens

A

aka group 7a elements are missing just one electron to fill their shell.

102
Q

refers to the ability of an atom to attract shared electrons in a covalent bond

A

Electronegativity

103
Q

in chemical reactions they tend to acquire electrons

A

halogens

104
Q

properties of metals

A

luster, malleable and ductile, conduct heat and electricity, tend to lose electrons

105
Q

able to be drawn out into a thin wire

A

ductile

106
Q

properties of nonmetals

A

dull,
brittle,
do not conduct heat or electricity well,
tend to gain electrons

107
Q

hard but liable to break or shatter easily

A

brittle

108
Q

hard but liable to break or shatter easily

A

brittle

109
Q

electronegativity is first proposed by

A

Linus Pauling

110
Q

when was electronegativity proposed

A

1932

111
Q

the most electronegative element; it pulls very strongly on the shared electrons in a covalent bond

A

flourine

112
Q

ability of an atom to donate electrons

A

elecpositivity

113
Q

for elements, it is the energy given off when an electron is added on the neutral atom.

A

electron affinity

114
Q

refers to the measure of the willingness of an atom to receive an electron

A

electron affinity

115
Q

is a measure of how much energy is required to remove an electron from a neutral atom

A

ionization energy

116
Q

the measure of the tendency of an atom to resist the loss of electron

A

ionization energy

117
Q

refers to the elements in a group

A

cogeners

118
Q

law of conservation of mass

A

matter can neither be created nor destroyed

119
Q

law of conservation of energy

A

energy cannot be created nor destroyed it can only be transformed from one form to another

120
Q

law of definite composition

A

a pure compound is always made up of the same constituent elements combined in a definite proportion by weight

121
Q

law of multiple proportion

A

when two elements react to form more than one compound, the different weights of the other are in the ratio of small whole numbers

122
Q

is any compoun that dissociates in water into H+ ions

A

acids

123
Q

is any substance that when dissolved in water, gives a solution a pH of less than 7

A

acids

124
Q

the combination of H+ and water (H30+) is known as

A

arrhenius theory of acids

125
Q

H30+ is known as

A

hydronium ion

126
Q

is any compound that dissociates in water to yield an H+ ion

A

arrhenius acid

127
Q

is any compound that is a proton donor when it dissolves in water

A

bronsted-lowry acid

128
Q

is any compound that is an electron pair acceptor

A

lewis acid

129
Q

properties of acids

A
  • acids conduct electricity in aqueous solutions
  • acids have a sour taste
  • acids turn blue litmus paper to red
  • acids have a ph between 0 and 7
  • acids neutralize bases
  • acids react with active metals to form hydrogen
  • acids react with oxides and hydroxides of metals tot form salts and water
130
Q

is any compound that dissociates in water into OH- ions.

A

bases

131
Q

it is a chemical compound that absorbs hydronium ions when dissolved in water (a proton acceptor)

A

bases

132
Q

is a special example of a base, where in an aqueous environment, hydroxide ions are donated

A

alkali

133
Q

is any compound that dissociates in water to yield an OH- ion

A

arrhenius base

134
Q

is any compound that is a proton acceptor when it dissolves in water

A

bronsted-lowry base

135
Q

is any compound that is an electron pair donor

A

lewis base

136
Q

properties of bases

A
  • bases conduct electricity in aqueous solutions
  • bases have a bitter taste
  • bases turn red litmus paper to blue
  • bases have a pH between 7 and 14
  • bases neutralize acids, forming salts and water
137
Q

the effect of an acid is to ______ in water, whereas bases _______

A

increase the hydronium ion concentration, reduce the concentration

138
Q

pH stands for

A

power of hydrogen

139
Q

is used to determine the number of hydrogen ions of a given substance.

A

pH

140
Q

acids pH range from

A

5.0 and below

141
Q

bases have a pH ranging from

A

8.5 and up

142
Q

is a chemical compound in which ions are held together in a lattice structure by ionic bonds

A

ionic compounds

143
Q

to form an ionic compound there needs to be atleast

A

one metal and one non-metal

144
Q

in ionic compound, the metal element is usually the ____ charge and the non-metal element in a ____ charge

A

positive, negative

145
Q

ionic compounds generally have high

A

melting and boiling points

146
Q

ionic compounds have good electrical conductivity when

A

molten or in solution

147
Q

when does ionic inorganic compounds form crystals

A

at room temperature, they become solids

148
Q

is a term used or ionic compounds composed of the cations and anions

A

salt

149
Q

why does salt need a positively charged cations and negatively charged anions

A

so that the product is neutral and without a net charge

150
Q

solutions of salts in water are called

A

electrolytes

151
Q

electrolytes as well as molten salts conduct

A

electricity

152
Q

salt that does not contain a hydroxide ion or a hydrogen ion

A

normal salt

153
Q

hydroxide ion

A

OH-

154
Q

hydrogen ion

A

H+

155
Q

is a salt that contain a hydroxide ion

A

basic salt

156
Q

salts that contain a hydrogen ion

A

acidic salts

156
Q

salts that contain a hydrogen ion

A

acidic salts

157
Q

is a chemical compound of oxygen with other chemical elements

A

oxides

158
Q

is a process by which one or more chemical substances are converted into one of more different chemical substances

A

chemical reaction

159
Q

types of chemical reactions

A
  • combination or synthesis
  • decomposition or analysis
  • single replacement
  • double replacement or metathesis
160
Q

what type of chemical reaction:

A + B –> AB

A

combination or synthesis

161
Q

what type of chemical reaction:

A B —> A+B

A

decomposition or analysis

162
Q

what type of chemical reaction:

A + BC —> AC + B

A

single replacement

163
Q

what type of chemical reaction:

AB + XY —> AY + XB

A

double replacement or metathesis

164
Q

is the math behind chemistry

A

stoichiometry

165
Q

is used to calculate masses, moles and percent within a chemical equation

A

stoichiometry

166
Q

the rules of determining stoichiometric relationships are based on

A

laws of conservation of mass and energy and the law of combining weights or volumes

167
Q

a homogeneous mixture of two or more substances

A

solution

168
Q

parts of solution

A

solute and solvent

169
Q

the dissolved substance or the part that has a lesser amount

A

solute

170
Q

the dissolving part of the solution or the part present in larger quantity

A

solvent

171
Q

is the ability of a compound to dissolve in another compound

A

solubility

172
Q

the measure of how much of a solute dissolves in a given amount of solvent

A

solubility

173
Q

factors influencing solubility

A
  • nature of solute and solvent
  • temperature
  • particle size of solid solute
174
Q

are properties of a solution such as melting point and boiling point change when other compounds are added

A

colligative properties

175
Q

colligative properties of solutions are properties that depend upon the

A

concentration of solute (molality)

176
Q

measure of the number of moles of solute in a solution corresponding to 1 kg or 1000g of solvent

A

molality

177
Q

factors that do not affect colligative properties

A
  • size of particles
  • mass of the particles
  • type of particles
178
Q

as the molality of the particles increases, it has the ff. effects on the solvent

A
  • the vapor pressure decreases
  • the boiling point increases
  • the freezing point decreases
179
Q

types of solution

A

saturated solution
unsaturated solution
supersaturated

dilute solution
concentrated solution

electrolyte
non-electrolyte

180
Q

no more solute can dissolve in the given amount of solvent

A

saturated solution

181
Q

the amount of solute dissolved in less than the solubility limit

A

unsaturated solution

182
Q

contains dissolved amount of solute exceeding the normal solubility limit

A

supersaturated

183
Q

comparatively has small amount of solute

A

dilute solution

184
Q

relatively has larger amount of solute

A

concentrated solution

185
Q

can conduct electricity, break into ions

A

electrolyte

186
Q

a compound that will dissolve in water to form a solution that does not conduct electricity due to ions not being produced

A

non-electrolyte

187
Q

are two liquids that do not dissolve in each other

A

immiscible liquids

188
Q

are compound that dissolve easily in water

A

hydrophilic compounds

189
Q

are compounds that do not dissolve easily in water

A

hydrophobic compounds

190
Q

all nonpolar compounds such as hydrocarbons are _____

A

hydrophobic

191
Q

is a measure of the quantity of an element or a compound.

A

mole

192
Q

a mole of an element will have a mass equal to the element’s ________

A

atomic weight

193
Q

a mole can be a

A

number quantity, a unit of mass, or a fixed volume of gas at STP

194
Q

Avogadro’s number

A

6.022x10^23

195
Q

a substance is numerically equal to its formula mass in grams

A

molar mass

196
Q

a mole (mol) is defined as the number of atoms in exactly ___g of ____

A

12g of carbon-12

197
Q

at stp, 1 mole of any gas occupies a volume of

A

22.4 L

198
Q

mole formula

A

grams/molecular weight

199
Q

1 mole is equal to _______ ions, atoms, molecules

A

6.022x10^23

200
Q

1 mole is equal to ______ of an element or compound

A

molar mass

201
Q

in a molecule or compound, it is the sum of the atomic weights of all the elements in the molecule

A

formula weight

202
Q

is generally the same as the formula weight whose units are expressed as g/mole (or amu)

A

molecular weight

GEAS: General Chemistry (2 decks)

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