Brainscape's Knowledge GenomeTM

Browse over 1 million classes created by top students, professors, publishers, and experts.


See full index

AP Chem > Final S1 > Flashcards

Final S1 Flashcards

You may prefer our related Brainscape-certified flashcards:
Periodic Table flashcards Chemistry 101 flashcards AP® Chemistry flashcards Organic Chemistry 101 flashcards
1
Q

What is the empirical formula?

A

The simplest whole number ration of elements

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
2
Q

What is the molecular formula?

A

Actual whole number ratio

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q

How do electrons exist around the nucleus?

A

In orbitals

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
4
Q

How do electrons become excited?

A

Photons of energy is added

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
5
Q

How do electrons return to ground state?

A

They release their added energy as photons (light)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
6
Q

When does ground state occur?

A

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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
7
Q

What is the order of orbitals?

A

S, p, d, f

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
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)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
9
Q

What is ionization energy?

A

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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

What is atomic radius/size?

A

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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
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)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
12
Q

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

A

Smaller

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
13
Q

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

A

Larger

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
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)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
16
Q

What is bond energy?

A

The energy required to break a bond

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
17
Q

What is an exothermic reaction?

A

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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
18
Q

What is an endothermic reaction?

A

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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
19
Q

What is an ionic bond?

A

A bond between a metal and nonmetal

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
20
Q

What is a covalent bond?

A

A bond between a nonmetal and nonmetal

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
21
Q

When is there the most lattice energy?

A

Biggest charge and smallest radius

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
22
Q

What is the electronegativity difference for a nonpolar colavent bond?

A

<.4

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
23
Q

What is the electronegativity difference for a polar covalent bond?

A

.4-1.8

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
24
Q

What is the electronegativity difference for an ionic bond?

A

> 1.8

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
25
Q

What is electronegativity?

A

The amount of energy needed for an atom to bond with another element

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
26
Q

What are the electronegativity trends and why?

A

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)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
27
Q

What is a dipolar/dipole moment?

A

A molecule that has a center of positive charge and a center of negative charge

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
28
Q

What do elements want to have?

A

A noble gas configuration

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
29
Q

What is lattice energy?

A

The amount of energy required to break a lattice

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
30
Q

What are the lattice energy trends and why?

A

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)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
31
Q

What do you do when elements are isoelectronic when caculating lattice energy?

A

Use the fact that the size decreases when there are MORE PROTONS in the nucleus (greatest atomic number is smallest)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
32
Q

What is the octet rule?

A

Each atom has 8 electrons around it in the lewis dot structures

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
33
Q

How do you calculate formal charge?

A

FC+ valence-dots/dashes

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
34
Q

What the bond angle for a linear electron geometry?

A

180

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
35
Q

What is the bond angle for a trigonal planar electron geometry?

A

120

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
36
Q

What is the bond angle for a tetrahedral electron geometry?

A

109.5

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
37
Q

What is the bond angle for a trigonal pyramidal molecular geometry?

A

<109.5

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
38
Q

What is the order for molecular geometry for two electron regions?

A

Linear

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
39
Q

What is the order for molecular geometry for three electron regions?

A

Trigonal planar, bent

40
Q

What is the order for molecular geometry for four electron regions?

A

Tetrahedral, trigonal pyramidal, bent

41
Q

What is the order for molecular geometry for five electron regions?

A

Trigonal bipyramidal, sawhorse, t-shaped, linear

42
Q

What is the order for molecular geometry for six electron regions?

A

Octahedral, square pyramidal, square planar, t-shaped, linear

43
Q

What is the hybridization order?

A

Sp, Sp2, Sp3, Sp3d, Sp3d2

44
Q

Why are metallic bonds like soup?

A

So they are malleable

45
Q

What is a intramolecular force?

A

A force that binds two atoms within a molecule together

46
Q

What is a intermolecular force?

A

The force between molecules or compounds

47
Q

What is a dipole-dipole attraction?

A

Attraction between a positive end and a negative end of two polar molecules

48
Q

What is a hydrogen bonding attraction?

A

A bond with F O N and H

49
Q

What is a london dispersion force attraction?

A

Weak attractions between every molecule

50
Q

What molecules have greater london dispersion forces? (Size wise)

A

Larger ones

51
Q

What are electrostatic (ionic) attractions?

A

Attractions between ionic compounds

52
Q

What is surface tension?

A

The tendency of liquid surfaces at rest to shrink into the minimum spaces possible

53
Q

What happens to water in surface tension?

A

It sticks to itself

54
Q

What is capillary action?

A

The tendency of a polar liquid to rise up a narrow tube

55
Q

What are the four types of solids?

A

Molecular (Covalent)
Ionic
Metallic
Network Covalent

56
Q

What are the four intermolecular forces?

A

LDF
H Bond
Dipole dipole
Ionic

57
Q

What is vapor pressure?

A

The pressure of vapor present at equilibrium

58
Q

How do intermolecular forces and vapor pressure relate?

A

Small intermolecular forces, high vapor pressure

59
Q

What happens at triple point?

A

All three phases exist

60
Q

What is the ideal gas law equation?

A

PV=nRT

61
Q

When do real gases behave like ideal gases?

A

At high temps and low pressures

62
Q

What are characteristics of a real gas?

A

Particles have volume
Energy is lost in collisions
Intermolecular forces

63
Q

What are characteristics of a ideal gas?

A

Particles have no volume
Collisions are elastic
No interactions between particles

64
Q

What is partial pressure?

A

The pressure that a particular gas would exert if it were alone in a container

65
Q

What is the mole fraction?

A

The number of moles of a substance to total moles in a given mixture

66
Q

What does kinetic molecular theory state?

A

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
Q

What size particles are faster?

A

The smaller ones

68
Q

What is the relationship between temp and kinetic energy?

A

As one increases, the other does as well

69
Q

What is a solution?

A

A homogeneous mixture of solute and solvent

70
Q

What is a solute?

A

A minor component of a liquid

71
Q

What is a solvent?

A

The major component of a liquid

72
Q

What is the universal solvent?

A

Water

73
Q

Why is water the universal solvent?

A

It is polar and ionic so it bonds with things easier

74
Q

What is hydration?

A

The dissolving of a substance in water

75
Q

What is dilution?

A

The process of adding water to a solution to achieve the desired molarity

76
Q

What is a stock solution?

A

A concentrated solution that is routinely diluted to form a particular desired solution

77
Q

What are examples of strong electrolytes?

A

Soluble salts, strong acids, strong bases

78
Q

What are examples of weak electrolytes?

A

Weak acids and weak bases

79
Q

What kind of electrolytes conduct electricity?

A

Strong ones

80
Q

What are examples of nonelectrolytes?

A

Covalent compounds (alcohols and sugars), insoluble salts

81
Q

What is the precipitate?

A

The solid that forms when two solutions are mixed

82
Q

What are first two the solubility rules for salts?

A

Nitrate (NO3) salts are soluble
Group one metals and ammonium are soluble

83
Q

How to determine if it is a soluble salt?

A

The rules

84
Q

How to determine if its a strong acid?

A

The seven strong acids

85
Q

What are the seven strong acids?

A

HBr
HI
HCl
HNO3
HClO3
HClO4
H2SO4

86
Q

What are acids?

A

Proton (H+) donors

87
Q

What are bases?

A

Proton (H+) acceptors

88
Q

What breaks apart?

A

Soluble salts, seven strong acids, strong bases

89
Q

How to determine if it is a strong base?

A

Group 1 or 2 metals with OH
NO3

90
Q

What happens to elements that loose electrons?

A

They are oxidized

91
Q

What happens to elements that gain electrons?

A

They are reduced

92
Q

What are the units for a zero order reaction?

A

Mol/L s

93
Q

What are the units for a first order reaction?

A

1/s

94
Q

What are the units for a second order reaction?

A

L/mol s

95
Q

What are the units for a third order reaction?

A

L^2/mol^2 s

96
Q

What are the five things that speed up a reaction?

A

Catalysts
Concentrations
Surface Area
Temperature
Pressure

97
Q

What is the reaction rate?

A

Change in concentration of a reactant or product per unit time

AP Chem (1 decks)

Brainscape helps you reach your goals faster, through stronger study habits.
© 2024 Bold Learning Solutions. Terms and Conditions