Fin Flashcards
(131 cards)
1
Q
Chemistry
A
The study of matter and the changes it undergoes
2
Q
Matter
A
anything that has mass and volume
3
Q
Mass
A
the amount of matter in an object
4
Q
Weight
A
the force of gravity acting on an object’s mass
5
Q
Kinetic Energy
A
-energy of motion
-measured by temperature
6
Q
Potential Energy
A
inversely related to kinetic energy
7
Q
Kinetic Theory of Matter/Kinetic Molecular Theory
A
matter is made up of particles which are in continual random motion
8
Q
States of Matter
A
-based on particle arrangement
-based on energy of particles and
-the distance between solid particles
9
Q
sublimation
A
solid to gas
10
Q
deposition
A
gas to solid
11
Q
plasma
A
-ionized gas
-excellent conductor of electricity
-affected by magnetic fields
-indefinite shape and volume
-most common state of matter
12
Q
point where something is a solid, liquid, and gas
A
triple point
13
Q
Pure Substances
A
-have a uniform and definite composition
-Elements
-Compounds (elements are bonded)
14
Q
Mixtures
A
-two or more substances mixed together
-blended
-no definite composition, cannot assign a fixed ratio
15
Q
Types of Mixtures
A
Heterogeneous
Homogeneous
16
Q
Heterogeneous
A
do not have a uniform composition
-parts of the mixture can be seen and removed
17
Q
Homogeneous
A
uniform composition
18
Q
Physical Properties
A
Properties that can be measured or observed without changing the identity or composition of a substance
-Ex. color, odor, texture etc
19
Q
Physical Changes
A
Changes in appearance without changing the composition of a substance
-Ex. cutting, breaking, pulverizing
Changes in state
-melting, freezing, boiling, subliming
20
Q
Chemical Properties
A
-Properties that indicate HOW a substance reacts with other substances
-only observed when the substance undergoes a chemical change
-Ex. combustible, flammable
21
Q
Chemical Changes (reactions)
A
-One or more substances react to form a completely new substance(s) with DIFFERENT chemical and physical properties
-Ex. rusting, corrosion, digestion, respiration
22
Q
Law of Conservation of Mass
A
matter cannot be created or destroyed
23
Q
Measurement
A
a type of observation
-two types, qualitative and quantitative
24
Q
Qualitative
A
descriptive
25
Quantitative
observation made with a measuring instrument and includes both a number and a unit
26
Accuracy
how close a measurement is to the true or accepted value
27
Precision
how close multiple measurements are to each other
28
% Yeild
expected/experimental x 100
29
% Error
abs(expected-experimental) all over expected then x 100
30
Significant Figure rules
-All non-zero digits are significant
-Leading zeros are never significant (zeros to the left)
-Captive zeros are always significant
-Trailing zeros are sometimes significant
31
Sig Figs- Addition and Subtraction
Answer is rounded to the same number of decimal places as the number used in the calculations with the least decimal places
-can only be as accurate as the least accurate value
32
Sig Figs- Multiplication and Division
Look at the total number of sig figs
Answer is rounded to the same number of decimal places as the number used in the calculations with the least s. figs
-Round at the END of calculations
33
Density?
D=M/V
34
Volume?
V=M/D
35
Mass?
M=VD
36
Dmitri Mendeleev
Organized elements by increasing atomic mass so that the elements in the same row had similar properties
-First periodic table
37
Henry Mosely
Rearranged the elements by increasing atomic number
-Current table
38
Periodic Law
When elements are arranged in order of increasing atomic number, there is a periodic pattern in their physical and chemical properties
39
Elements in the same group have _______ properties.
similar
40
Elements in the same period have _______ properties
different
41
Metals
-left of the staircase
-lustrous
-malleable and ductile
-good conductors
*Includes aluminum
42
Nonmetals
-right of the staircase
-non-lustrous
-brittle
-poor conductors
*Includes hydrogen
43
Metalloids
touch staircase and have properties of both metals and nonmetals
44
Semiconductors
normally do not conduct electricity, but will at high temps or when certain substances are added
45
Democritus
First person to think about atoms
-"atomos"
-believed matter was composed of indivisible particles
46
John Dalton
1. All elements are composed of indivisible particles called atoms
2. Atoms of the same element are identical. Atoms of any one element are different from those of another
3. Atoms of different elements mix or combine in whole number ratios
4. Chemical reactions occur when atoms separate, join, or rearrange. In a chemical reaction, atoms of one element NEVER change into another
47
Cathode Ray Tube Experiment
JJ Thompson
-In a tube was an inert gas and two plates, one positive and one negative
-therefore particles must have a positive and a negative charge
48
JJ Thompson
-Discovered the electron
-Cathode Ray Tube Experiment
-Plum Pudding Model
49
Ernest Rutherford
-Gold foil experiment
-discovered the nucleus
50
Gold foil expriment
Rutherford
-Shot high-energy beam of alpha particles into gold foil
Observations:
-Most went through, a few particles were deflected at small anges
-Very rarely particles were deflected at large angles
Conclusions:
-atom is mostly empty space
-alpha particles came close to small and positively charged particles (deflected at small angles)
- hit very small, very dense, positively charged nucleus (deflected at large angles)
51
Eugene Goldstein
discovered the proton
52
James Chadwick
discovered the neutron
53
relative mass of electron
1/1840
54
Atomic number
number of protons in an element
55
Average atomic mass
weighted average of all an elements' isotopes
56
Mass number
number of protons and neutrons
57
number of neutrons (formula)
mass #- atomic #
58
Isotopes
same # of protons, different # of neutrons
59
AMU
Atomic mass units- 1/12 mass of a carbon-12 atom
60
Formula for average atomic mass
Atomic mass(sub1) x (%/100) + atomic mass (sub2) x (%/100).....
61
Mass spectrometer/spectrometry
of spots hit=# of isotopes
-heavier isotopes hit lower, vice versa
62
charge
charge=protons - electrons
63
Cations
positive charge, typically metals
64
Anions
negative charge, typically nonmetals
65
Quantum Mechanical Model
We cannot pinpoint where an electron is, but we can give the probability of where it is
66
electron configurations
show how electrons are distributed within an atom
67
How many energy levels are there?
7 (periods)
68
s
spherical
69
p
dumbell
70
d
clover
71
f
double clover
72
Aufbau Principle
electrons enter sublevels lowest to highest energy
73
Pauli Principle
Atomic orbitals can hold only 2 electrons at most, and they must have opposite spins
74
Hund's Rule
In a sublevel with more than one orbital, put one electron in each orbital before putting 2e- in any one orbital
75
Quantum numbers
used to describe the distribution of electrons in atoms
76
n
-principle quantum number
-the average distance of electrons to the nucleus
77
l
-angular momentum quantum number
-shape of the orbital
-n-1=l
-ex. when n=1, l=1-1=0
-e. when n=3, l=3-1=1 and 0 (s & p sublevels)
78
m(sub l)
-magnetic quantum number
-orientation of the orbital in 3D space
- -l
79
m(sub s)
electron spin quantum number
-+1/2 or -1/2
-up or down spin
80
To count valence e- ______
look at the highest numbered energy level, the add e- together
81
How to write NG
pick closest noble gas before element, write config for element after NG in brackets
-ex. K= K: [Ar] 4s^1 Ar=1s2 2s2 2p6 3s2 3p6
82
Isoelectronic
if two elements have the same # of e-, they are isoelectronic
83
What is the relationship between frequency and wavelength?
inversely proportional
84
What is the relationship between energy and frequency?
directly proportional
-the higher the frequency, the more energy
85
What is the equation is for finding the energy of a photon (particle)?
E = hf = hc/λ. Here h = 6.626*10-34
86
What is the equation for finding the energy for an energy level?
E(n) = −1/n2 × 13.6eV
87
what 3 well-known phenomena prove light's ray-like properties?
-reflection
-refraction
-scattering
88
Wave
a vibrating disturbance by which energy is transmitted
89
Wavelength
the distance between identical points on a wave
90
Frequency
the number of waves that pass through a point in one second
91
Amplitude
the height of the wave from the mid-line of the wave to the crest or trough
92
Node
point of zero amplitude
93
Speed of Waves
c=λv
c= speed of light
λ= wavelength
v= frequency
94
Light as a Ray
James Maxwell
95
Max Planck
-light as a particle
-discovered that atoms and molecules emit energy in discrete quantities called quanta
-E=hv
-v=frequency
-h=Planck's constant
96
E=hv
energy and frequency are directly related/directly proportional
97
c=λv
wavelength and frequency are indirectly related/inversely proportional
98
Einstein
-studied photoelectric effect
-light contains "tiny lumps" of light particles called photons
99
dual nature of light
"Light is a collection of particles (photons) moving through space as electromagnetic waves"
100
______ came up with the solution to Rutherford's paradox by using Rutherford's and ______ work to design a model for the hydrogen atom
1. Bohr
2. Planck
101
Bohr was right in that ______
but wrong _____
-there are energy levels which prevent the atom from collapsing upon itself
-in their behavior
102
Energy from wavelength
hc/lambda
103
wavelength of a frequency
lambda=v/f
v=wave velocity
104
frequency
v/lambda
105
Louis Victor de Broglie
suggested all matter could be described as having wave-like properties
-lambda=h/mv
106
Heisenberg's Uncertainty Principle
"It is impossible to know both the position and energy of an electron in an atom simultaneously- we can only know one with leaving the other"
107
Schrödinger
-developed equations that took into account the particle and wave-like nature for an e-, the solutions to which are called *wave functions*
-Quantum numbers are used to solve
-wave mechanical model
108
Atomic Radius
1/2 distance between the nuclei of two like atoms
109
the radius of an atom is dependent upon what two factors
1. nuclear charge
2. Distance between electrons and nucleus
110
Period trend for atomic size
decreases left to right
111
Group trend for atomic size
decreases further down the table
112
Ionization energy
the amount of energy required to remove an electron from a gaseous atom- to make cationic
113
What two factors does IE depend on
-Distance between the valence electrons and the nucleus
-Effective nuclear charge (# of p+)
114
Coulomb's law
describes the force of attraction
-FoA=(charge)(charge) all over r squared
115
fluorine is the ____ attractive element
most
116
Francium is the ______ attractive element
least
117
group trend for IE
IE decreases down a group due to the increasing distance of the valence electrons from the nucleus
118
period trend for IE
IE increases as you move across a period due to an increased effective nuclear charge
119
cations are always ______ than their natural selves
smaller
-neutral is the largest form for cations
120
anions are always ______ than their natural selves
larger
121
Electronegativity
the tendency or ability for an element to attract electrons when chemically combined with another element
122
group trend for EN
decreases moving down
123
period trend for EN
increase across the table
124
IE and EN are _________ __________ to the radius
inversely proportional
125
What are the two types of bonding
ionic and covalent
126
ionic
the transfer of electrons
-one element loses and the other gains e-
127
covalent
involves a sharing of e- atoms will share in order to reach a stable electron configuration
128
Octet rule
8 e- is great
129
Atoms will lose or gain electrons in order to become _______ with a noble gas
isoelectronic
130
Ionic compounds are also known as _____ generally and certain compounds are called _______
1. salts
2. crystals
131
Properties of Ionic Compounds
-Very strong
-Always solids at room temp
-Very high melting and boiling points
-metal and nonmetal
-Don't normally conduct electricity
