GENCHEM Flashcards
1
Q
Anything that has mass and volume.
A
Matter
2
Q
Can be described by using physical and
chemical properties.
A
Matter
3
Q
These are
properties that can be observed or measured
A
Physical Properties
4
Q
These are properties that determine whether or not a substance will react chemically.
A
Chemical Properties
5
Q
Does not depend on the size or amount of the sample
A
Intensive Properties
6
Q
Depends on the size or amount of the sample.
A
Extensive Properties
7
Q
Physical or Chemical Property:
Flammability
A
Chemical
8
Q
Physical or Chemical Property:
Mass
A
Physical
9
Q
Physical or Chemical Property:
Length
A
Physical
10
Q
Physical or Chemical Property:
State
A
Physical
11
Q
Physical or Chemical Property:
Density
A
Physical
12
Q
Physical or Chemical Property:
Reactivity
A
Chemical
13
Q
Physical or Chemical Property:
Conductivity
A
Physical
14
Q
Intensive or Extensive Property:
Color
A
Intensive
15
Q
Intensive or Extensive Property:
Volume
A
Extensive
16
Q
Intensive or Extensive Property:
Volume
A
Extensive
17
Q
Intensive or Extensive Property:
Odor
A
Intensive
18
Q
Simplest substance, made up of atom
A
Element
19
Q
Made up of more than one type of atom
A
Compound
20
Q
Uniform composition
A
Homogenous Mixture
21
Q
Different composition
A
Heterogeneous Mixture
22
Q
States that each element is composed of extremely small particles called atom.
A
Dalton’s Billiard Ball Model
23
Q
Compounds form by combining atoms
A
Dalton’s Billiard Ball Model
24
Q
Year of Dalton’s Billiard Ball Model
A
1803
25
States that the atom is made up of negative electrons that float in a sphere of positive charge like plums in a pudding
Thomson’s Plum Pudding Model
26
Discovered electron via cathode ray experiment in 1897
J. J. Thomson
27
Discovered isotopes in 1913
J. J. Thomson
28
Discovered the nucleus of a gold atom with his “gold foil” experiment.
Ernest Rutherford
29
States that the atom is mostly empty space
Rutherford’s Nuclear Model
30
States that nucleus surrounded by orbiting electrons at different energy levels
Bohr’s Planetary Model
31
Electrons have definite orbits
Bohr’s Planetary Model
32
Positive Charge
Proton
33
Neutral Charge
Neutrons
34
Negative charge
Electron
35
Number of protons in nucleus.
Atomic Number
36
The number of _________ determines identity of the element.
Proton
37
Number of protons + neutrons
Mass Number
38
Atoms of the same element with varying number of neutrons
Isotopes
39
Carbon has ______ naturally occurring isotopes with C-12 having the highest percent abundance
Three
40
True or False:
Different isotopes have different mass numbers because the number of neutrons is different.
True
41
States that the elements were arranged in
groups of 3’s or triads like iron,
cobalt and nickel which are alike
in many properties, so with chlorine, bromine and iodine
Law of Triad
42
Law of Triad
Johann Wolfgang Dobereiner
43
Elements are arranged in groups of 8’s like from lithium to sodium and from fluorine to chlorine. These elements have similar properties and are seven elements apart.
Law of Octaves
44
Law of Octaves
John Newlands
45
Recognized the repeating pattern or the periodic behavior among elements
Julius Lothar Meyer
46
Studied the relationship of the atomic volume and the relative atomic mass of 28 elements
Julius Lothar Meyer
47
Formulated the Periodic Law
Dmitri Mendeleev
48
The seven horizontal rows in the periodic table are called
Periods
49
Has 2 elements
corresponding to 2 electrons in the **s** sublevel
Period 1
50
Has 8 elements
corresponding to 8 electrons in the **s** and **p** sublevels
Period 2 & 3
51
Have 18 elements corresponding to 18 electrons in the **s**, **p** and **d** sublevels
Period 4 & 5
52
Has 32 elements corresponding to 32 electrons in the **s**, **p**, **d**, **f** sublevels
Period 6
53
Still incomplete but elements fill up **s**, **p**, **d** and **f** sublevels.
Period 7
54
The vertical columns in Periodic Table
Groups or Families
55
Alkali Metals Group
Group 1A
56
Alkaline Earth Metals Group
Group 2A
57
Halogens Group
Group 7A
58
Boron Family
Group 3A
59
Carbon Family
Group 4A
60
Nitrogen Family
Group 5A
61
Oxygen Family
Group 6A
62
Each element in the group has a completely filled set of **s** and **p** orbitals
Noble Gases
63
All colorless and exhibit little or no reactivity
Noble Gases
64
Other words for Noble Gases
Inert Gases
65
Columns 1B to 8B or B family/group
Transition Elements
66
Additional horizontal rows below compromise two groups of elements
Inner Transition Elements
67
Lantahanum in 6th period, rare-earth elements
Lanthaniods
68
Actinium in 7th period, heavy rare elements
Actinoids
69
Most ideal gas element
Helium
70
The average distance between nucleus and the valence electron
Actomic Size
71
Other word for Atomic Size
Atomic Radius
72
In Atomic Size Group Trend, as you go down a column, atomic size ________
increases
73
In Atomic Size Periodic Trend, as you go from right to left, atomic size ________
increases
74
In Ionic Radius:
Cationic Radius < Neutral Atomic Radius
(Al3+ < Al)
True
75
In Ionic Radius:
Anion Radius > Neutral Atomic Radius
(O2- > O)
True
76
The ability of the atom to donate electrons.
Metallic Property
77
In Metallic Property Group Trend, as you go down a column, metallic property _________.
increases
78
In Metallic Property Periodic Trend, as you go right to left, metallic property _________.
increases
79
Tendency of an atom to react.
Reactivity
80
In Reactivity Group Trend, as you go down a column, reactivity _________.
increases
81
In Reactivity Periodic Trend, as you go right to left, reactivity _________.
increases
82
The amount of energy required to remove an electron from an atom or ion.
Ionization Energy
83
In Ionization Group Trend, as you go down a column, ionization _________.
decreases
84
In Ionization Periodic Trend, as you go right to left, ionization _________.
decreases
85
The change in energy when an electron is accepted by a gaseous atom to form an anion.
Electron Affinity
86
In Electron Affinity Group Trend, as you go down a column, electron affinity _________.
decreases
87
In Electron Affinity Periodic Trend, as you go right to left, electron affinity _________.
decreases
88
The relative ability of an atom of an element to attract or gain electrons.
Electronegativity
89
In Electronegativity Group Trend, as you go down a column, electronegativity _________.
decreases
90
In Electronegativity Periodic Trend, as you go right to left, electronegativity _________.
decreases
91
Is Mg > Ca > K > Fr arranged according to increasing atomic size?
Yes
92
Which of the following elements is more electronegative:
Cl, S, or Mg?
Cl
93
Which of the following elements is more reactive: Li, Rb, or Fr?
Li
94
Which of the following elements has the
higher ionization energy, Br or Cu?
Br
95
Which has a larger ionic size (Na+ or Mg2+)
Na+
96
**SUMMARY:**
**!!INCREASES!!**
Atomic Size - Metallic Property - Reactivity
**!!DECREASES!!**
Ionization Energy - Electron Affinity - Electronegativity
OK
97
The orbitals of an atom must be filled up in increasing energy levels.
Aufbau Principle
98
No two electrons in an atom can have the same set of quantum numbers and an atomic orbital must contain a maximum of two electrons with opposite spins.
Pauli’s Exclusion Principle
99
The most stable arrangement of
electrons in subshells is the one with more parallel spins.
Hund’s Rule of Multiplicity
100
The average distance of the electron from the nucleus in a particular orbital. (n)
Principal Quantum Number
101
It tells the shape of the
orbital. (l)
Azimuthal / Angular
Momentum Quantum Number
102
Describes the
orientation of orbital. (ml)
Magnetic Quantum Number
103
Shows the spin of electrons. (ms)
Spin Quantum Number
104
Formed by actual electron-transfer where one of the reacting atoms loses one or more electrons and the other atom gains on or more electrons.
Ionic Bonding
105
Formed by electron sharing, usually between atoms of non-metals.
Covalent Bonding
106
Metal to Non-Metal bonding
Ionic Bonding
107
Non-metal to Non-metal bonding
Covalent Bonding
108
In
which two or more substances (either elements or compounds)
react to form one compound.
Composition reaction
109
This reaction is also known as combination, direct union or synthesis.
Composition reaction
110
In which one compound decomposes to form two or more new substances. Usually heat is necessary to cause this reaction
to take place.
Decomposition reaction
111
This reaction is also known as analysis.
Decomposition reaction
112
In which a metal replaces another metal ion from a solution or a non metal replaces a less
active non metal in a compound.
Single replacement reaction
113
This reaction is also called displacement or substitution.
Single replacement reaction
114
In which two compounds react to form two new compounds. This involves exchange of ion pairs.
Double decomposition
reaction
115
This reaction is also called exchange reaction or metathesis.
Double decomposition
reaction
116
In which the
substance that is oxidized is called the reducing agent, while
the substance that is reduced is called the oxidizing agent.
Oxidation-Reduction
Reactions (REDOX
REACTIONS)
117
A + B --> AB
Composition reaction / Combination / Direct Union / Synthesis.
118
AB --> A + B
Decomposition reaction / Analysis
119
AX + B --> BX + A
AX + Y --> AY + X
Single replacement reaction / Displacement / Substitution.
120
AX + BY --> AY + BX
Double decomposition
reaction / Exchange
reaction / Metathesis.
121
6.02x10^23
Avogadro’s Number
122
The ratio of the total mass of each element to the total mass of one mole of the compound (MM)
multiplied by 100%.
Percent Composition
123
Gives the simplest ratio of the number of
moles of atoms.
Empirical Formula
124
Gives the actual ratio of the number of
moles of atoms in a mole of the compound.
Molecular Formula
125
Homogeneous
mixture of 2 or more substances.
Solution
126
Parts of Solution
Solute & Solvent
127
Dissolving Medium
Solvent
128
Dissolved Substance
Solute
129
Ability of a solvent
to dissolve a salt at a particular temperature.
Solubility
130
Solution where solvent can still
dissolve the solute.
Unsaturated Solution
131
Solution where the
solvent can’t dissolve the solute and
need to be heated for it to be dissolved.
Supersaturated Solution
132
Solution where a solvent can’t no longer dissolve a given solute at a given temperature.
Saturated Solution
133
The relative amount of solute present in a
solution.
Concentration of Solution
