PART 1 Flashcards
(128 cards)
1
Q
The science that describes matter—its properties, the changes it undergoes, and the energy changes that accompany those processes
A
Chemistry
2
Q
Chemistry is also called the ___ science.
A
Central
3
Q
Branch of chemistry that deals with metals, minerals, and stuff mostly found on the periodic table.
A
Inorganic Chemistry
4
Q
Branch of chemistry that talks about hydrocarbons and their derivatives.
A
Organic Chemistry
5
Q
Detection and identification of substances present (qualitative analysis) or amount of each substance (quantitative analysis)
A
Analytical Chemistry
6
Q
Branch of chemistry that deals with the processes in living organisms
A
Biochemistry
7
Q
Branch of chemistry that covers the behavior of matter
A
Physical chemistry
8
Q
Anything that has mass and occupies space
A
Matter
9
Q
Measure of the quantity of matter
A
Mass
10
Q
Amount of space
A
Volume
11
Q
The capacity to do work or to transfer heat
A
Energy
12
Q
Energy in motion
A
Kinetic Energy
13
Q
Energy at rest
A
Potential Energy
14
Q
Reaction where heat is released.
A
Exothermic
15
Q
Reaction where heat is absorbed.
A
Endothermic
16
Q
Ice melting is an example of ___ reaction (energy change).
A
Endothermic
17
Q
Is energy matter?
A
No
18
Q
State of matter that fills any container completely and highly compressible.
A
Gas
19
Q
____ properties can be observed or measured without changing the identity of the substance.
A
Physical
20
Q
____ properties are exhibited by matter as it undergoes changes in composition.
A
Chemical
21
Q
Which of the following is a chemical property of matter?
A. Silver is a shiny metal that conducts electricity very well.
B. Sulfur is a yellow powder.
C. A dry piece of paper burns.
D. Pure water, for example, has a density of 0.998 g/cm^3 at 25°C.
A
C. A dry piece of paper burns.
22
Q
___ properties are dependent on the amount of substance.
A
Extensive
23
Q
____ properties are independent of the amount of substance.
A
Intensive
24
Q
Which of the following is an EXTENSIVE property of matter?
A. Hardness
B. Size
C. Melting point
D. Color
A
B. Size
25
If the property is unchanged by altering the sample size, it's an ____ property.
Intensive
26
A change where one or more substances are used up and one or more new substances are formed.
Chemical Change
27
A change where there is no change in chemical composition.
Physical Change
28
Which of the following exhibits a chemical change?
A. lce cream melting
B. Making a sand castle
C. A Macbook falling out of a window
D. Fireworks Exploding
D. Fireworks Exploding
29
TRUE OR FALSE
A physical change may suggest that a chemical change has also taken place.
True
30
CLASSIFICATION OF MATTER
It may be separated into pure substances by physical methods (e.g. distillation, filtration).
Mixture
31
CLASSIFICATION OF MATTER
It cannot be separated into simpler substances by physical methods.
Pure substance
32
CLASSIFICATION OF MATTER
Components are NOT distinguishable
Homogeneous mixtures
33
CLASSIFICATION OF MATTER
It has a fixed composition (e.g. 100% ethanol).
Pure substance
34
CLASSIFICATION OF MATTER
It has a single phase and the same composition throughout (i.e. same amount in any area).
Homogeneous mixtures
35
CLASSIFICATION OF MATTER
It has variable composition (e.g. 70%, 80%, or 95% ethanol in water).
Mixture
36
CLASSIFICATION OF MATTER
Preferred for drugs
Homogeneous mixtures
37
CLASSIFICATION OF MATTER
It does NOT have the same composition throughout (i.e. different amount in various areas) and has multiple phases.
Heterogeneous Mixtures
38
CLASSIFICATION OF MATTER
Components are distinguishable.
Heterogeneous Mixtures
39
CLASSIFICATION OF MATTER
It can be decomposed into simpler substances by chemical changes
Compounds
40
CLASSIFICATION OF MATTER
Water broken into hydrogen and
oxygen gases via electrolysis.
Compounds
41
CLASSIFICATION OF MATTER
It consists of atoms of two or more different elements bound together.
Compounds
42
CLASSIFICATION OF MATTER
It cannot be decomposed into simpler substance by chemical changes.
Elements
43
CLASSIFICATION OF MATTER
It consists of only one kind of atom.
Elements
44
Most abundant element in the universe
Hydrogen
45
The smallest unit that retains the properties of an element.
Atom
46
Theory that states that all matter is composed of atoms and these cannot be made or destroyed.
Dalton’s Theory
47
The number of protons in the nucleus of an atom that also determines its identity.
Atomic Number (Z)
48
The sum of the number of protons and the number of neutrons in its nucleus.
Mass Number (A)
49
Atoms of the same element with different
masses.
Isotopes
50
They are atoms containing the same number of protons but different numbers of neutrons.
Isotopes
51
Same mass number, different atomic numbers.
Isobars
52
Same number of neutrons, different atomic numbers.
Isotones
53
Represents the composition of the nucleus
Nuclide Symbol
54
Formula for calculating the number of neutrons given the mass number and atomic number.
No.of Neutrons = Mass Number — Atomic Number
55
The weighted average of the masses of an element's isotopes.
Atomic Weight
56
TRUE OR FALSE:
Atomic weights are fractional numbers, not integers.
True
57
Coined the greek word "atomos" meaning uncuttable
Leucippus and Democritus
58
Theorized atoms as solid indivisible spheres
Leucippus and Democritus
59
Matter is made up of four elements (earth, fire, air, water).
Aristotle
60
Atom as solid sphere but NOT indivisible.
John Dalton
61
Who made the Solid Sphere (Billiard Ball) Model?
John Dalton
62
Elements of a chemical compound are held together by electrical forces.
Humphry Davy
63
Relationship between the amount of electricity used in electrolysis and the amount of chemical reaction that occurs.
Michael Faraday
64
Coined the term "electrons" from electron ions
George Stoney
65
Performed the Cathode-Ray Tube Experiment that provided the most convincing evidence of electrons
Joseph John Thomson
66
Joseph John Thomson developed the ___ model of the atom.
Plum pudding
67
The Oil-drop Experiment was performed by ___.
Robert Millikan
68
The Oil-drop Experiment determined the charge of ___.
Electrons
69
Saturn-like model was made by ___.
Hantaro Nagaoka
70
The Canal Rays Experiment was performed by ___.
Eugen Goldstein
71
Positive rays, or positive ions, are created when the gaseous atoms in the tube lose electrons.
Canal Rays Experiment by Eugen Goldstein
72
The Scattering Experiment was performed by ___.
Ernest Rutherford
73
Atoms consist of very small, very dense positively charged nuclei surrounded by clouds of electrons at relatively large distances from the nuclei.
The Scattering Experiment by Ernest Rutherford
74
Positive charge localized in the nucleus
Nuclear model (from The Scattering Experiment by Ernest Rutherford)
75
He studied X-rays given off by various
elements.
“The number of protons in the nucleus of an atom determines its identity; this number is known as the atomic number of that element.”
H.G.J. Moseley
76
Bombardment of beryllium with high-energy alpha-particles produced neutrons
J. Chadwick
77
Described the electron of a hydrogen atom as revolving around its nucleus in one of a discrete set of circular orbits
Niels Bohr
78
Proposed the idea of the wave-like nature of electrons
Louis de Brogli
79
When an electron is excited from a lower energy level to a higher one, it absorbs a definite (quantized) amount of energy.
Bohr’s Planetary Model
80
Quantum mechanics is based on the ___ properties of matter.
Wave
81
What principle states that for electrons, it is not possible to determine the exact momentum and the exact position at the same moment in time?
Werner Heisenberg’s Uncertainty Principle
82
It estimates the position of electrons and quantifies energy levels.
Erwin Schrodinger’s Wave Equation
83
A region of space in which the probability of finding an electron is high.
Atomic Orbitals
84
The Modern Atomic Model is developed by ___.
Erwin Schrodinger
85
The Modern Atomic Model is also called ___ or ___.
Electron Cloud Model
Quantum Mechanical Model
86
QUANTUM NUMBERS
Represents the distance of the electron from the nucleus
Principal QN (n)
87
QUANTUM NUMBERS
Higher principal QN (n), ___ energy
Higher
88
QUANTUM NUMBERS
The orbital in principal QN (n) refers to the ___ or ___.
Shell or energy level
89
QUANTUM NUMBERS
Angular momentum QN (l) is also called ___ or ___ angular momentum QN.
Azimuthal or Orbital
90
QUANTUM NUMBERS
The orbital in angular momentum QN (l) refers to the ___ or ___.
Subshell or sublevel
91
QUANTUM NUMBERS
Angular momentum QN (l) is ___ less than the principal QN (n).
One (n-1)
92
QUANTUM NUMBERS
Identify the shape of the orbital based on the angular momentum QN (l).
0
Spherical (s-orbital)
93
QUANTUM NUMBERS
Identify the shape of the orbital based on the angular momentum QN (l).
1
Dumb-bell (p-orbital)
94
QUANTUM NUMBERS
Identify the shape of the orbital based on the angular momentum QN (l).
2
Cloverleaf (d-orbital)
95
QUANTUM NUMBERS
Identify the shape of the orbital based on the angular momentum QN (l).
3
Complex (f-orbital)
96
QUANTUM NUMBERS
The orbital in magnetic QN (ml) refers to the ___.
Specific orbital
97
QUANTUM NUMBERS
It refers to the orientation in space of the orbital.
Magnetic QN (ml)
98
QUANTUM NUMBERS
____ QN (___) is the positive and negative values of the angular momentum QN (l).
Magnetic QN (ml)
99
QUANTUM NUMBERS
____ is used for each individual electron only.
Spin QN (ms)
100
QUANTUM NUMBERS
Value for clockwise direction of spin
+1/2
101
QUANTUM NUMBERS
Value for counter-clockwise direction of spin
-1/2
102
This describes the distribution of electrons.
Electron Configuration
103
It describes the number and arrangement of electrons in orbitals, subshells, and shells in an atom.
Electron Configuration
104
Atom in its lowest energy, or unexcited, state.
Ground state
105
What principle states that orbitals fill in order of increasing energy, from lowest to highest?
Aufbau principle
106
No more than two electrons can occupy each orbital, and if two electrons are present, they must have opposite spins. What principle is this?
Pauli Exclusion Principle
107
A single electron will occupy an empty orbital first before pairing.
Hund’s Rule
108
PERIODIC TABLE OF ELEMENTS
Arranged the periodic table based on chemical properties
Dimitri Mendeleev
109
PERIODIC TABLE OF ELEMENTS
Arranged the periodic table based on physical properties
Lothar Meyer
110
PERIODIC TABLE OF ELEMENTS
Elements are now arranged in the periodic table in order of ___.
Increasing atomic number
111
PERIODIC TABLE OF ELEMENTS
“The properties of the elements are periodic functions of their atomic numbers.” What do you call this law?
Periodic Law
112
PERIODIC TABLE OF ELEMENTS
Vertical columns in the periodic table
Groups or families
113
PERIODIC TABLE OF ELEMENTS
Horizontal rows in the periodic table
Periods
114
PERIODIC TABLE OF ELEMENTS
Defined as half of the distance between the nuclei of neighboring atoms in the pure element
Atomic Radii (Size)
115
PERIODIC TABLE OF ELEMENTS
Expressed in Angstroms (1A = 10^-10 m)
Atomic Radii (Size)
116
PERIODIC TABLE OF ELEMENTS
The energy required to remove an electron from a gas-phase atom
lonization Energy (IE)
117
PERIODIC TABLE OF ELEMENTS
The energy change that occurs when an electron is attached to an atom in the gas phase to form a negative ion.
Electron Affinity (EA)
118
PERIODIC TABLE OF ELEMENTS
Measure of the relative tendency of an atom to attract electrons to itself when it is chemically combined with another atom
Electronegativity (EN)
119
PERIODIC TABLE OF ELEMENTS
Metalloids are ___ at lower temperatures but become ___ at higher temperatures.
Insulators, Conductors
120
PERIODIC TABLE OF ELEMENTS
Metalloids that are semiconductors
Silicon
Germanium
Antimony
121
PERIODIC TABLE OF ELEMENTS
Non-metals are good heat ___ except carbon.
Insulators
122
PERIODIC TABLE OF ELEMENTS
Metals have ___ electrical conductivity that ___ with increasing temperature.
High
Decreases
123
PERIODIC TABLE OF ELEMENTS
PERIODIC TRENDS: Upper-right corner or Lower-left corner
Atomic radius
Lower-left corner
124
PERIODIC TABLE OF ELEMENTS
PERIODIC TRENDS: Upper-right corner or Lower-left corner
Metallic character
Lower-left corner
125
PERIODIC TABLE OF ELEMENTS
PERIODIC TRENDS: Upper-right corner or Lower-left corner
Ionization energy
Upper-right corner
126
PERIODIC TABLE OF ELEMENTS
PERIODIC TRENDS: Upper-right corner or Lower-left corner
Electronegativity
Upper-right corner
127
PERIODIC TABLE OF ELEMENTS
PERIODIC TRENDS: Upper-right corner or Lower-left corner
Electron affinity
Upper-right corner
128
PERIODIC TABLE OF ELEMENTS
PERIODIC TRENDS: Upper-right corner or Lower-left corner
Non-metallic character
Upper-right corner
