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Regents Flashcards

(96 cards)

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0
Q

Temperature

A

Average kinetic energy

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1
Q

Amount of energy required to steal the outermost electron

A

Ionization energy

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2
Q

Particles of an ideal gas are separated by great distances, compared to their size

A

Kinetic molecular theory

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3
Q

What happens when a bond is broken

A

Energy is absorbed

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4
Q

What happens when a bond is formed

A

Energy is released

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5
Q

What does a catalyst do

A

Creates an alternate pathway, increasing the rate of the reaction by lowering the activation energy

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6
Q

Where does oxidation and reduction occur?

A

Oxidation-anode

Reduction-cathode

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7
Q

Same molecular formula but different structural formula

A

Isomer

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8
Q

Amount of attraction for electrons in a chemical bond

A

Electronegativity F or closest to fluorine

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9
Q

Difference between potential energy of the products and potential energy of the reactants

A

Heat of the reaction

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10
Q

Atoms that bond with each other to form chains, rings, or networks

A

Carbon atoms

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11
Q

Electrical energy to chemical energy

A

Electrolytic cell

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12
Q

MaVa=MbVb

A

Titration

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13
Q

Dense (+) charged in the center of empty space (protons & neutrons)

A

The nucleus

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14
Q

Mass of protons, neutrons, and electrons…

A

Protons: 1.0073amu. +
Neutrons: 1.0087amu. 0
Electrons: 0.0005amu. -

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15
Q

Atoms with the same number of protons but different number of neutrons

A

Isotope

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16
Q

Weighted average of all isotopes

A

Average atomic mass

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17
Q

A nucleus that is unstable

A

Radioactive

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18
Q

What determined the stability of a nucleus

A

The number of neutrons vs the number of protons

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19
Q

Change in the identity (#P) In a nucleus

A

Transmutation

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20
Q

If unstable nucleus undergoes a…

A

Transmutation to become stable

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21
Q

For nuclei with more than 83 protons

A

Alpha decay

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22
Q

For nuclei with too many neutrons

A

Beta decay

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23
Q

For nuclei with too many protons

A

Positron

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24
The time required for half of a radioactive sample to become stable
Half life
25
A large nucleus breaks releasing energy
Fission Nuclear power
26
2 small nuclei fuse together release tons of energy
Fusion Sun/bomb
27
Isotopes with short half lives used to treat and protect health problems ( 131-I: thyroid disorders) ( 60-Co: finding and fighting cancer)
Medical tracers
28
Determines the age of fossils ( 238-U: date the earth) ( 14-C: dates organic fossils)
Radioactive dating
29
Fission, fission, atomic bomb, radiation | Matter converted to energy
Artificial transmutation
30
How do you determine the charge of an atom?
Number of protons - number of electrons
31
#p>#e 1P 0e Charge=1+
Cation
32
#p=#e 1p 1e Charge=0
Neutral atom
33
#p<#e 1p 2e Charge=1-
Anion
34
Atoms with a charge due to more or less electrons
Ion
35
What are the energy levels in a Bohr model
1st=2 electrons 2nd=8 electrons 3rd=18 electrons 4th=32 electrons
36
If heat or electrics is added what happens to electrons
They jump to an excited state
37
How is light produced
Excited by energy electron hops up to an excited state then falls back done to ground state and energy is released as light
38
Partial rainbow that only shows transitions between Es and Gs
Line emission spectrum
39
Shows all colors in the rainbow
Continuous spectrum
40
Revised version of the Bohr model
Wave-mechanical model
41
Regions of probably electron density (electron location)
Electron move in ORBITALS
42
Group of same type of atoms
Element
43
``` High Melting/boiling point High density Shiny High conductivity of heat and electricity Malleable and ductile ```
Metal
44
``` Low melting and boiling point Low density Dull Poor conductor Brittle ```
Non-metal
45
``` Middle melting/boiling point Middle density Middle luster Middle conductivity Middle hardness ```
Metalloid
46
Elements in which two atoms are bonded
Diatomic elements | BrOFINClH
47
Size of an atom in pm from the nucleus to the outer shell, size increases down a group due to pull of electrons
Atomic radius
48
Size of an ion compared to it's atom
Ionic radius
49
Why are cations smaller than anions
Less electrons than protons
50
High atomic radius =?
Low ionization energy
51
Mutual attraction between two atoms to form a stable octet of valence electrons
Chemical bond
52
What are the three types of bonds
Covalent: 2 nM ^ electronegativity Ionic: M and nM high and low electronegativity Metallic: 2 M Low electronegativity
53
The ability of an atom to attract electrons in a bond
Electronegativity
54
Decrease the size=?
Increase electronegativity
55
Steps for Lewis structures
1. Make an electron check list 2. Put atom with the lowest EN that isn't H in the center 3. Place all other atoms around 4. Place electrons around to for stable octets
56
Based on difference in EN
Polarity
57
``` Strong Hard Not conductivity in solid Conductivity in water Dissolves in water High mp/bp ```
Ionic
58
``` Medium Soft Not conductivity in solid or water Dissolves in h2o Medium mp/bp ```
Polar covalent
59
``` Medium Soft Not conductivity in solid or water Doesn't dissolve in water Low mp/bp ```
No polar covalent
60
``` Weak Hard Conductive in solid Doesn't dissolve in water High mp/bp ```
Metallic
61
What indicates a chemical reaction
Heat or light is given off A color change occurs A gas is given off A solid precipitates out
62
Will of the atoms of the left my so be also on the right
Law of conservation of mass
63
Ability of an atom to react and form an ion
Chemical activity
64
2 become 1
Synthesis
65
1 breaks apart
Decomposition
66
Element + compound--> new compound + new element
Single displacement
67
AB+CD--> AD + CB
Double displacement
68
CxHy + O2--> Co2(g) + H2O(g)
Combustion
69
The simplest whole number ratio of Atoms for a family of compounds
Empirical formula
70
Mols=grams ------- GFM
Gram to mole conversions
71
Energy from a machine
Mechanical
72
Energy from a feeling of warmth
Thermal
73
Energy from movement and bonds
Chemical
74
Energy from light
Light
75
Energy from moving electrons
Electrical
76
Energy from fission reactions
Nuclear
77
Transfer of thermal energy from hot to cold
Heat
78
Amount of energy needed to raise a 1.0 g of a sample by 1° C or 1K
Specific heat
79
Below 1 J/g/k
Heats up quickly, cools down quickly
80
Above 1 J/g/k
Heats up slowly, cools down slowly
81
Atoms and molecules can react if they collide with proper speed and orientation
Collision theory
82
Rate influencing factors
1) Temperature 2) Concentration 3) Surface area 4) Nature of reactions
83
Gasses dissolve at...
Low temp | high pressure
84
Real gases act most ideal at...
High temp | Low pressure
85
Adding more solvent to a concentrated solution
Dilutions
86
Physical properties of a solution that depend on only amount not what it is
Colligative properties
87
Factors of colligative properties
Love freezing point | High boiling point
88
Use double displacement
Arrhenius reaction
89
A compound that acts as both an acid and a base
Amphoteric
90
An experiment in which a known amount of acid is fully neutralized by an unknown amount of base
Titration
91
Rules for assigning oxidation numbers
1) oxi # for all elements is 0 2) oxi # for single atom ions is their charge 3) oxi # for group 1 is +1 and group 2 is +2 4) oxi # for o is always -2 5) oxi # for H is +1 except when bonded to a group one or 2 metal (-1)
92
One product of saponification
Soap
93
Yeast
Fermentation
94
Which organic reaction includes an acid
Esterification
95
Form long chains long chains from small molecules
Polymerization

Chemistry (1 decks)

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