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AP Chem > Final S1 > Flashcards

Final S1 Flashcards

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1
Q

What is the empirical formula?

A

The simplest whole number ration of elements

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2
Q

What is the molecular formula?

A

Actual whole number ratio

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3
Q

How do electrons exist around the nucleus?

A

In orbitals

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4
Q

How do electrons become excited?

A

Photons of energy is added

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5
Q

How do electrons return to ground state?

A

They release their added energy as photons (light)

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6
Q

When does ground state occur?

A

When electrons are in their lowest possible energy level (closest to nucleus)

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7
Q

What is the order of orbitals?

A

S, p, d, f

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8
Q

What is the trend for ionization energy and why?

A

Increases from left to right (more vallance electrons)
Increases from bottom to top (fewer energy shells so things are closer to nucleus)

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9
Q

What is ionization energy?

A

The minimum energy required to remove the most loosely bound electron of an isolated gaseous atom

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10
Q

What is atomic radius/size?

A

The average distance from the center of the nucleus to the outermost electron

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11
Q

What is the trend for atomic radius and why?

A

Decreases from left to right across a period (more protons, stronger pull inward)
Increases from top to bottom within a group (more energy levels)

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12
Q

Is the atomic radius of a positive ion smaller or larger than the atomic radius of the element?

A

Smaller

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13
Q

Is the atomic radius of a negative ion larger or smaller than the radius of the element?

A

Larger

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14
Q

What is electron affinity?

A

The amount of energy released when an electron attaches to the neutral atom or molecule in the gaseous state to form an anion

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15
Q

What is the trend for electron affinity and why?

A

Increases left to right (closer to noble gas, so more likely to accept that atom to get to noble gas)
Increases bottom to top (more exothermic and adding an electron releases more energy)

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16
Q

What is bond energy?

A

The energy required to break a bond

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17
Q

What is an exothermic reaction?

A

A reaction that releases energy from the system in the form of heat

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18
Q

What is an endothermic reaction?

A

A reaction that the system absorbs energy from its surrounding in the form of hear

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19
Q

What is an ionic bond?

A

A bond between a metal and nonmetal

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20
Q

What is a covalent bond?

A

A bond between a nonmetal and nonmetal

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21
Q

When is there the most lattice energy?

A

Biggest charge and smallest radius

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22
Q

What is the electronegativity difference for a nonpolar colavent bond?

A

<.4

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23
Q

What is the electronegativity difference for a polar covalent bond?

A

.4-1.8

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24
Q

What is the electronegativity difference for an ionic bond?

A

> 1.8

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25
What is electronegativity?
The amount of energy needed for an atom to bond with another element
26
What are the electronegativity trends and why?
Increases upward (less orbitals, tighter rings around nucleus, more energy to pry apart) Increases to the right (more energy is needed to complete the vallance shell)
27
What is a dipolar/dipole moment?
A molecule that has a center of positive charge and a center of negative charge
28
What do elements want to have?
A noble gas configuration
29
What is lattice energy?
The amount of energy required to break a lattice
30
What are the lattice energy trends and why?
Decreases down a group (more energy levels so weaker attractions) Across a period (elements that give up electrons get smaller and elements that gain get bigger)
31
What do you do when elements are isoelectronic when caculating lattice energy?
Use the fact that the size decreases when there are MORE PROTONS in the nucleus (greatest atomic number is smallest)
32
What is the octet rule?
Each atom has 8 electrons around it in the lewis dot structures
33
How do you calculate formal charge?
FC+ valence-dots/dashes
34
What the bond angle for a linear electron geometry?
180
35
What is the bond angle for a trigonal planar electron geometry?
120
36
What is the bond angle for a tetrahedral electron geometry?
109.5
37
What is the bond angle for a trigonal pyramidal molecular geometry?
<109.5
38
What is the order for molecular geometry for two electron regions?
Linear
39
What is the order for molecular geometry for three electron regions?
Trigonal planar, bent
40
What is the order for molecular geometry for four electron regions?
Tetrahedral, trigonal pyramidal, bent
41
What is the order for molecular geometry for five electron regions?
Trigonal bipyramidal, sawhorse, t-shaped, linear
42
What is the order for molecular geometry for six electron regions?
Octahedral, square pyramidal, square planar, t-shaped, linear
43
What is the hybridization order?
Sp, Sp2, Sp3, Sp3d, Sp3d2
44
Why are metallic bonds like soup?
So they are malleable
45
What is a intramolecular force?
A force that binds two atoms within a molecule together
46
What is a intermolecular force?
The force between molecules or compounds
47
What is a dipole-dipole attraction?
Attraction between a positive end and a negative end of two polar molecules
48
What is a hydrogen bonding attraction?
A bond with F O N and H
49
What is a london dispersion force attraction?
Weak attractions between every molecule
50
What molecules have greater london dispersion forces? (Size wise)
Larger ones
51
What are electrostatic (ionic) attractions?
Attractions between ionic compounds
52
What is surface tension?
The tendency of liquid surfaces at rest to shrink into the minimum spaces possible
53
What happens to water in surface tension?
It sticks to itself
54
What is capillary action?
The tendency of a polar liquid to rise up a narrow tube
55
What are the four types of solids?
Molecular (Covalent) Ionic Metallic Network Covalent
56
What are the four intermolecular forces?
LDF H Bond Dipole dipole Ionic
57
What is vapor pressure?
The pressure of vapor present at equilibrium
58
How do intermolecular forces and vapor pressure relate?
Small intermolecular forces, high vapor pressure
59
What happens at triple point?
All three phases exist
60
What is the ideal gas law equation?
PV=nRT
61
When do real gases behave like ideal gases?
At high temps and low pressures
62
What are characteristics of a real gas?
Particles have volume Energy is lost in collisions Intermolecular forces
63
What are characteristics of a ideal gas?
Particles have no volume Collisions are elastic No interactions between particles
64
What is partial pressure?
The pressure that a particular gas would exert if it were alone in a container
65
What is the mole fraction?
The number of moles of a substance to total moles in a given mixture
66
What does kinetic molecular theory state?
Particles do not have weight Particles are in constant motion Particles exert no forces Average kinetic energy of the gas is directly proportional to the temperature of the gas
67
What size particles are faster?
The smaller ones
68
What is the relationship between temp and kinetic energy?
As one increases, the other does as well
69
What is a solution?
A homogeneous mixture of solute and solvent
70
What is a solute?
A minor component of a liquid
71
What is a solvent?
The major component of a liquid
72
What is the universal solvent?
Water
73
Why is water the universal solvent?
It is polar and ionic so it bonds with things easier
74
What is hydration?
The dissolving of a substance in water
75
What is dilution?
The process of adding water to a solution to achieve the desired molarity
76
What is a stock solution?
A concentrated solution that is routinely diluted to form a particular desired solution
77
What are examples of strong electrolytes?
Soluble salts, strong acids, strong bases
78
What are examples of weak electrolytes?
Weak acids and weak bases
79
What kind of electrolytes conduct electricity?
Strong ones
80
What are examples of nonelectrolytes?
Covalent compounds (alcohols and sugars), insoluble salts
81
What is the precipitate?
The solid that forms when two solutions are mixed
82
What are first two the solubility rules for salts?
Nitrate (NO3) salts are soluble Group one metals and ammonium are soluble
83
How to determine if it is a soluble salt?
The rules
84
How to determine if its a strong acid?
The seven strong acids
85
What are the seven strong acids?
HBr HI HCl HNO3 HClO3 HClO4 H2SO4
86
What are acids?
Proton (H+) donors
87
What are bases?
Proton (H+) acceptors
88
What breaks apart?
Soluble salts, seven strong acids, strong bases
89
How to determine if it is a strong base?
Group 1 or 2 metals with OH NO3
90
What happens to elements that loose electrons?
They are oxidized
91
What happens to elements that gain electrons?
They are reduced
92
What are the units for a zero order reaction?
Mol/L s
93
What are the units for a first order reaction?
1/s
94
What are the units for a second order reaction?
L/mol s
95
What are the units for a third order reaction?
L^2/mol^2 s
96
What are the five things that speed up a reaction?
Catalysts Concentrations Surface Area Temperature Pressure
97
What is the reaction rate?
Change in concentration of a reactant or product per unit time

AP Chem (1 decks)

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