1.0 Flashcards
(210 cards)
1
Q
All matter is composed of discrete units called atoms
A
Atomic Theory
2
Q
Atoms are invisible and atoms of elemets are identical
A
Solid Sphere
3
Q
Solid Sphere. Who and When
A
John Dalton, 1803
4
Q
Electrons are scattere throughout a spherical cloud of positively charged particles
A
Plum Pudding/Thomson Model
5
Q
Plum Pudding. Who and when
A
JJ Thoms on , 1904
6
Q
Atom is mainly empty space with a positively charged center. Electrons revolve a predicatble path
A
Nuclear/Rutherford Model
7
Q
Negatively charged electrons revolve around the positively charged
A
Planetary/Bohr’s model
8
Q
Planetary model who and when
A
Niels Bohr, 1913
9
Q
Electrons are found in clouds of probability called orbitals. Exact location is impossible to determin. Still widely accepted as the most accurate mdoel of the atom.
A
Quantum
10
Q
Quantum. Who and when
A
Erwin Schrodinger, 1926
11
Q
Who discovered electrons
A
JJ Thomson
12
Q
Who discovered Protons
A
Ernest rutherford
13
Q
Who discovered Neutron
A
James Chadwick
14
Q
Number of protons
A
Atomic Number
15
Q
Number of electrons
A
number of protons
16
Q
Number of neutrons
A
mass number - atomic number
17
Q
ability of an atom to donate an electron
A
Metallic Property
18
Q
Average distance between the nucleus and the valence electron
A
Atomic Size
19
Q
Tendency of atom to react
A
Reactivity
20
Q
energy required to remove an electron from an atom
A
Ionization Energy
21
Q
Change in energy when a gaseous atom/ion gains an electron
A
Electron affinity
22
Q
Abilityof an atom to attract or gain an electron
A
Electronegativity
23
Q
Started the development of the Periodic Table, arranging elements by increasing atomic mass
A
Dmitri Mendeleev
24
Q
first discovered radioactivity
A
Antioine Bequerel
25
Discovered the elements radium and polonium
Pierre and Marie CurieD
26
Determined that atomic number, not atomic weight is the correct basis for ordering elements
Henry Moseley
27
atomic weight of the middle elements of the triad was roughly the average of the other two elements
Law of triads
28
identified the law of Triads
Johann Dobereiner
29
observing that every eighth element had similar properties when elements were arranged by atomic weight
Law of Octaves
30
proposed the Law of Octaves
John Newlands
31
recognized periodic trends between atomic volume and atomic weight
Lothar Meyer
32
defined elements as pure substance that cannot be broken down into simpler substances laying the groundwork for modern chemistry
Robert Boyle
33
father of Modern Chemistry
Antoine Lavoisier
34
developed a modern system of naming chemical substances, identified and named oxygen and hydrogen
Antoine Lavoisier
35
established law of Conservation of Mass
Antoine Lavoisier
36
Vertical colums; similar valence electrons and chemical characteristices
Groups
37
Horizontal Rows; same number of electron shells
periods
38
determines how a particular atom reacts (same numebr of valence electrons = reacts in the same similar manner
valence electrons
39
Group 1A to 8A
Main Group elements
40
another name for main group elements
representative elements
41
Groups 3 to 12.
Transition elements
42
characterized by their ability to form multiple oxideation staes and have colored compounds
transition elements
43
metals are all soid at room temp except
mercury
44
usually shiny, very dense, high melting points
metal
45
in chemical rections, they readily lose electrons to form positive ions
Metals
46
brittle, dull, low melting points
nonmetals
47
poorconductors of heat and electricuity
nonmetals
48
in chemical reactions they tend to gain electrions forming negative ions
nonmetals
49
exhibit both properties of metals and nonmetals
semimetals
50
can conducts electricity better than insulatos but not as well as conductors
semiconductors
51
highlyreactive metals due to their larger atomic radii and low ionization energies. soft, silvery and can be easity cut
alkali metals (group 1)
52
reactive metals but less so than alkali metals. they commonly form compounds like oxides and hydroxides
alkaline earth metals
53
characterized by their ability to form complex ions and are effective catalysts
transition metals (groups 3-12)
54
highly reactive nonmetals, known for forming salts when reacting with metals
halogens
55
unique group because it concludes all states of matter at room temperature and notable for containing 4 out of seven diatomic elements
Halogens(group7a/17)
56
Diatomic particles in halogens
F2, Cl2, Br2, I2
57
Inert, colorless and oderless gases with a complete valence electron shell, making them extremely stable and mostly nonreactive. they are used in lighhting and as inert atmospheres in chemical reaction
Noble gases (group 8a)
58
rare earth metals, known for their magnetic and phosphorescent properties
lanthanides
59
elements used in electronics, lasers and strong magents
lanthanides
60
radioactive elements many of which are synthetic
actinides
61
notable for their use in nuclear energy
uranium and thorium
62
nonmetal, diatomic gas that can act like an alkali metal by losing one electron or like a halogen by gaining one electron
hydrogen
63
a highly reactive non-metal essential for combustion and respiration.
oxygen
64
most abundant element on earth
oxygen
65
can form stable bonds with itslef and other elements
carbon
66
backbone of organic chemistry and life
carbon
67
increase as you move down, drecrease as you move across
atomic radius
68
most electronegative element
fluorine
69
have an elctronegativity rating of 0 due to their inherent stability, preventing them from forming bonds with other atoms
noble gases
70
more tightly bound and require more energy to be removed
electrons closer to the nucleus
71
how easily and element can lose an electron
metallic character
72
most reactive chemical, reacting explosively with water and igniting spontaneously in air
cesium
73
rare that its properties ARE LARGELY OBSERVED
francium
74
tendency of an element to gain an electron in chemical reactions
nonmetallic character
75
most reactive nonmetal as it is not found in nature as free element and reacts explosively with many substance
fluorine
76
formed by the transfer of electron between metals and nonmetals
ionic compounds
77
formed by the sharing of electrons between nonmetals
covalent (molecular) compounds
78
ions made up of multiple atoms bonded covalently but carrying an overall charge
polyatomic ions
79
common polyatomic ions
sulfate and ammonium
80
compounds that release H+ ions in solutions
Acids
81
named with "hydro-" prefix and "-ic"suffix
binary acids
82
named based on the polyatomic ion "-ate" becomes "-ic acid" and "-ite" becomes "-ous acid"
oxyacids
83
acids containing hydrogen, oxygen and another element
oxyacids
84
containing hydrogen and one other element
binary acids
85
compounds that release OH- ions in a solution
bases
86
names by stating the metal cation followed by hydroxide
bases
87
ionic compounds formed from the neutralization reaction between an acid and a base
salts
88
named by combining the names of the cation and the anion
salts
89
compounds primarily made of carbon and hyddrogen atoms, often containg oxygen, nitrogen and other elements
organic compounds
90
named based on the number of carbon atoms and the types of bonds
organic compounds
91
branch of chemistry that studies and explians the behavior of subatomic particles like electrons and light
quantum chemistry
92
has oscillating electric and magnetic fields in planes and perpendicular to each other in the direction of propagation
electromagnetic radiation
93
distance between two consecutive peaks or troughs
wavelength
94
distance from origin to crest
amplpitude
95
number of waves/cycles that pass a point per unit time
frequency
96
shows the inverse relationship of frequency and wavelength
speed
97
speed of light
3x10^-8 m/s
98
speed of sound
343 m/s
99
postulated that light and other electromagnetic waves can be quanticized
max planck
100
dicrete packets of energy
quanta
101
quantify the wavelength when the atom transitions from the exited phase to ground phase
Rydberg's equation
102
result of excitation of the atoms and releasing excess energy by emitting light of various wavelegths
atomic spectrum of hydrogen
103
concluded that when photons are shone at a metal surface, some electrons can be knocked off in the metal structure
Albert Einstein (Photoel;ectric Effect)
104
energy that will drive away electrons from the metal surface
Kinetic Energy
105
minimum energy to remove electrons from the metal surface
work function
106
postulated that electrons can behave as waves
louis de broglie
107
used to distingush the probability of finding electrins in 3D space accoriding to mathematical function
Qauntum Mechamic Model
108
regions in space without electron density
nodes
109
adress of an electron in an atom
quantum numbers
110
main energy level or the distance of electrons from the nucleus
Principal
111
Energy subshells or the shape of the orbitals
Azimuthal
112
Number of orbitals in subshells or the possible orientation of orbitals in space
magnetic
113
movement of electrons around its own axis
Spin
114
arrangement of electrons in the orbital of an atom
electron configuration
115
also called the building up principle
Aufbau Principle
116
orbitals are filled with electron in increasing energy
aufbau principle
117
most stable arrangement of electrons in subshells is the one with more parallel spis
hund's rule of maximum multiplicity
118
same eneegy orbital, upward electrons should be filled up first before the downward electrons
hund's rule of maximum multiplicity
119
no two electrons can have same set of four quantum numbers
pauli's exclusion principle
120
lowest energy arrangement of electrons in the orbital of an atom
ground state
121
allowed arrangments other than the ground state
excited state
122
electrons with the highest pricipal quantum number
valence electrons
123
electrons closer to the nucleus
core electrons
124
all the number of electrons of the highest energy level
valence electron of configuration
125
species with the same electron of configuration
isoelectronic
126
usual electron configuration
condensed
127
all electrons of every subshells are expanded with two electrons each
expanded
128
simplified condensed electron configuration using the previous nearest noble gas to the element
Noble gas
129
driving force of chemical bonding
attain stable electronic configuration
130
metal - nonmetal
ionic
131
nonmetal - nonmetal
covalent
132
hydrogen - electronegative atom
hydrogen bond
133
metal - metal
metalliv bond
134
interactions between charged molecules
electrostatic
135
this type of interaction arises when there is induction of a dipole in the molecules
induction
136
london forces or van der waals forces and exist mostly in covalent molecules
dispersion
137
interaction between the hydrogen and an electronegative element where there is no electron exchange leading to weak bonding between molecules
hydrogen bonds
138
used for predicting the number of bonds formed by most elements in theire compounds
lewis electron dot symbols
139
consist of the chemical symbol for an element surrounded by dots that reperesent its valence electrons
lewis dot symbol
140
who and when. lewis electron dot symbol
Gilbert N. Lewis (20th century)
141
states that atoms tent to gain, lose or share electrons in order to achieve a stable configuration with eigth valence electrons
octet rule
142
elements that can accomodate more than eight electrons on their valence shell, such as elements from the third point onwards
expanded octet
143
elements that have fewer that eight electrons in their valence shell, such as hydrogen and helium
incomplete octet
144
elements that have an odd number of valence electrons, such as nitrogen. therefore, all of these options deviate the octet rule
odd number octet
145
the three-dimensiona arrangement of all the atoms in a given molecule
molecular geometry
146
- the number of domains attached to a central atom (atoms and lone pairs)
Steric number
147
- in a bond is caused by electronegativity differences between the bonded atoms.
Polarity
148
● are highly compressible and have low densities
Gas molecules have weak IMFAs
149
● are slightly compressible and have high densities
Liquid molecules have stronger IMFAs
150
● are almost incompressible and have high densities
Solid molecules have very strong IMFAs
151
a _______represents a quantity of a number, the same way a “dozen” does.
mole
152
Shows how many atoms of each element are in a compound
● Molecular Formula
153
the simplest or most reduced ratio of atoms in a compound
Empirical Formula
154
- the percent by mass of each element in a compound
Percentage Composition -
155
involve the interaction of chemicals to form new substances
Chemical Reactions
156
two or more substance combine to form one product
Combination Reaction
157
combination reaction: Metal + Nonmetal
Binary Compound
158
Combintaion Reaction: ● Nonmetal + Oxygen
Nonmetal Oxide
159
Combination Reaction: ● Metal + Water
Metal Hydroxide (base)
160
cobination reaction: ● Nonmetal oxide + Water
Oxyacid (acid
161
combination reaction: ● Metal oxide + Nonmetal oxide
salt
162
a compound is decomposed to form two or more substances
Decomposition Reaction
163
Decomp Rxn: salt + water
Hydrates
164
Dec Rxn: Carbonates + H2O (g)
+ CO2
● IA Bicarbonate
165
Dec Rxn: Metal oxide + H2O (g)
+ CO2
● IIA Bicarbonates
166
Dec Rxn: Metal oxide + CO2
● Carbonates
167
Dec Rxn: Chlorine + Oxygen
● Chlorates
168
Dec Rxn: Metal + Oxygen
● Metal oxide
169
Dec Rxn: Hydrogen + Oxygen
● Water
170
more active metal can displace a less active metal, while a less active one can’t displace the more active.
Displacement Reaction
171
the positive ions exchange partners with the negative ions to form two new compounds.
Metathesis (double displacement)
172
● All neutralization reactions involving acids and bases are actually
metathesis reactions.
173
used to describe the quantitative relationships between the reactants and products in a chemical reaction.
Stoichiometry
174
● The reactant that is completely consumed during a chemical reaction
Limiting Reactant
175
● Once used up, the reaction stops, even if other reactants are still available.
Limiting Reagent
176
● The reactant(s) that remain after the reaction has completed.
Excess Reactant
177
Present in small amount
Dissolved substance
solute
178
Does not change its phase in the formation of solution
Dissolving medium
solvent
179
solvent can still dissolve the solute
Unsaturated Solution
180
if a solvent can’t no longer dissolve a given solute at a given temperature
Saturated Solution
181
if the solvent can’t dissolve the solute and need to be heated for it to be dissolved
Supersaturated Solution
182
All nitrates, bicarbonates, chlorates
and compounds containing alkali metal ions and ammonium
ion.
Soluble Compounds
183
All halides except that
of Ag+, Hg2 2+ and Pb2+
Soluble Compounds
184
All sulfates except that of Ag+, Ca++, Sr++, Ba++
and Pb++
Soluble compounds
185
All carbonates, phosphates, chromates,
and sulfides except that of alkali metal ions and ammonium
ion.
insoluble compounds
186
All hydroxides except that of alkali metal ions and Ba++
insoluble compounds
187
Chemical reactions tend to move towards a dynamic equilibrium in which both reactants and products are present but have no further tendency to undergo net change.
Chemical Equilibrium
188
Describes the relationship between the concentrations of reactants and products in a chemical reaction at equilibrium. It is expressed by the equilibrium constant (K)
Equilibrium Law
189
Ratio of the concentration of products to the concentration of the reactants, each raised to their respective stoichiometric coefficients.
Equilibrium Constant (KC)
190
represents the equilibrium constant measured in moles per liter (concentration).
Kc
191
represents the equilibrium constant calculated using the partial pressures of gasses.
Kp
192
If a system at equilibrium is subjected to a change in concentration (C), pressure (P), or temperature (T), the system will adjust itself to counteract the disturbance and restore a new equilibrium.
Le Chatelier’s Principle
193
the energy required to separate a nucleus into neutrons and protons,
Nuclear Binding Energy
194
emission of protons, neutrons, and electromagnetic waves from the nucleus of an unstable atom
Radioactivity
195
process of losing energy through light emission of an unstable nucleus
Radioactive Decay
196
determines whether the atom will undergo radioactive decay
Nuclear Stability
197
Even number of
protons and neutrons
stable
198
Magic number of protons and neutrons:
2, 8, 20, 28, 50 82, 126
199
Neutron to proton ratio > 1
unstable
200
it has a positive charge, very low penetrating power and very high ionizing power.
Alpha Decay
201
it has a negative charge, intermediate penetrating and ionizing power.
beta decay
202
it has a no charge, very high penetrating power and very low ionizing power.
gamma decay
203
also called as the decay time
hal-life
204
uses the concept of first-order reaction to determine the time wherein the sample has lost half of its content.
half-life
205
contains and control nuclear fission (splitting apart of atoms) that release energy in the form of heat
Nuclear Reactors
206
a common nuclear fuel which is capable of producing nuclear reaction and it can readily undergo fission
Uranium-235
207
contains the fuel elements and moderator; it is where the nuclear reaction occurs
Core
208
reduces speed of neutrons; usually light-water
Moderator
209
control the rate of nuclear reaction by adsorbing excess neutrons; made up of Cadmium and Boron
Control Rods
210
a heat exchanger that is used to produce the steam
steam generator
