Thou Shalt Not Forget Flashcards
1
Q
Compounds are separated into elements by?
A
Chemical Changes
2
Q
Mixtures are separated into elements by?
A
Physical changes
3
Q
Filtering separates mixtures based on differences in?
A
Particle size, large particles are trapped on the filter paper and the soluble compound goes through it
4
Q
Distillation separates mixtures based on differences in?
A
Boiling point
5
Q
What component moves up the farthest in paper chromatography?
A
The most similar in polarity to the “mobile phase”
6
Q
What is conserved in chemical and physical changes?
A
Mass
7
Q
When reading a volume of a liquid in a container, you can estimate by?
A
Reading in between the graduated markings, giving one more sig fig
8
Q
Measuring devices from least precise to most precise?
A
Beaker, graduated cylinder, volumetric flasks, and burette
9
Q
Density equals?
A
Mass/ volume
10
Q
The % composition for a pure compound?
A
Does not change
11
Q
Gas mixtures are homogeneous because of?
A
The constant random motion of the particles
12
Q
Gases are compressible because of?
A
The large space between the particles
13
Q
Gas pressure is caused by?
A
Collisions of particles with the walls of the container
14
Q
More collisions=?
A
More pressure
15
Q
Pressure and volume are?
A
Inversely related
16
Q
Temperature and volume are?
A
Directly related
17
Q
Temperature and pressure are?
A
Directly related
18
Q
Doubling the volume of the container will?
A
Cut the pressure in half
19
Q
Heating a rigid container will?
A
Increase the pressure of the gas
20
Q
A heated balloon will?
A
Expand
21
Q
PV=
A
nRT
22
Q
Temperature=
A
Kelvin
23
Q
Volume=
A
Liters
24
Q
Pressure=
A
atm
25
Gas constant, R=
.0826
26
One mole of an ideal gas at STP=
22.4 liters
27
Gas pressure and number of moles are?
Directly related
28
If you double the moles of gas in a container?
The pressure will double
29
Molar mass=
dRT/P
30
Density=
g/L
31
The more molar mass a gas has?
The slower it moves at a given temperature
32
Temperature=
Average Kinetic Energy
33
Gases at the same temperature have?
The same average kinetic energy
34
Collecting a gas by water displacement?
P(total)=P(dry gas) + P(water vapor)
35
Real gases behave most like an ideal gas at?
High temperature and low pressure
36
The more polar a gas is and the larger a gas is, the more it will?
Deviate from ideal behavior
37
Small, nonpolar gases are?
The most ideal
38
An electron is where when farther away from the nuclues?
A higher energy level
39
An electron with less Coulombic attraction to the nucleus is?
Easier to remove, it has a lower 1st ionization energy
40
Moving across a row on the periodic table, the Z eff increases, therefore the valence electrons?
Are more attracted to the nucleus, the atomic radius decreases and the ionization energy increases
41
When reading a PES graph, the higher the peak?
The more electrons there are in that sublevel
42
A larger binding energy means that?
The electrons are closer to the nucleus
43
What are the ionization levels?
1s2 2s2 2s6 3s2 3p6 4s2 3d10 4p6
44
When writing the electron configuration for a cation, remove the?
Valence electrons first, p orbital and s orbital, then d orbita
45
Isotopes of the same element have?
Same number or protons, different number of neutrons
46
Mass spectroscopy graphs measure?
Atomic masses of isotopes
47
Elements in the same group (vertical columns) have?
Similar chemical and physical properties
48
Metals are on what side of the zig-zag line?
Left side
49
Nonmetals are on what side of the zig-zag line?
Right side
50
Cation are smaller than anions because?
You are removing valence electrons farther from the nucleus
51
Anions are bigger that cations because?
Adding extra electrons increases electron-electron repulsions
52
Covalent bonds are formed between?
Two nonmetals sharing electrons
53
Ionic bonds are formed when?
A metal transfers electrons to a nonmetal and the opposite charges attract
54
The greater the electronegativity difference between two atoms?
The more polar the bond becomes
55
Combustion reactions make?
CO2 and H2O
56
H2, O2, N2, Cl2, Br2, I2, F2
Diatomic elements, when in a compound, their number of atoms can vary
57
Empirical formula rhyme?
% to mass, mass to mole, divide by small, times til whole.....get the simplest whole # ratio of the moles (or atoms) in the compound
58
The molecular formula for a compound is?
A whole # multiple of the empirical formula ratio
59
Percent yield=
(experimental)/(theoretical)
60
%error=
(experimental-theoretical)/ theoretical
61
The amount of product for a reaction is determined by?
The limiting reactant
62
Carbon makes a total of how many bonds in a compound?
4
63
Bond angle, 4 domains?
109.5 degrees
64
Bond angle, 3 domains?
120 degrees
65
Bond angle, 2 domains?
180 degrees
66
Hybrid orbitals, 4 domains?
sp3
67
Hybrid orbitals, 3 domains?
sp2
68
Hybrid orbitals, 2 domains?
sp
69
Asymmetrical molecules=
Dipoles don't cancel, polar molecule
70
Symmetrical molecules=
Dipoles cancel, nonpolar molecule
71
Single bond=
Sigma
72
Double bond=
Sigma + pi bond
73
Triple bond=
Sigma + two pi bonds
74
What is lattice energy?
The energy needed to break an ionic bond in a compound, increases as ion's charge increases, decreases as radii of ions increase (deduced from Coulomb's Law)
75
What does formal charge involve?
Comparing the # of valence electrons an atom has to the # of electrons around it in the Lewis structure ("split" the bonded electrons evenly between the atoms)
76
When drawing Lewis Dot Structure, you should?
Obey the octet rule first, use formal charge if necessary, put extra electrons on the larger central atom, and make double or triple bonds if you have too few electrons
77
First IMF
London Dispersion
78
Second IMF
Dipole-dipole
78
Third IMF
Hydrogen Bonding
79
Fourth IMF
Ion-dipole
80
All molecules have what force
London Dispersion Forces
81
What makes LDF stronger?
Larger molecule, Larger electron cloud, more polarizable
82
Larger Electron cloud= more LDF = ?
More polarizable
83
All polar molecules contain what forces?
Dipole-dipole, which is stronger when more polar
84
Hydrogen bonds are between?
NOF, and another hydrogen bonded to NOF in a compound
85
Boiling points and melting points increase as?
IMF increases
86
As IMF increases, vapor pressure and volatility?
Decreases
87
Molecular solids have what melting and boiling points?
Low ones
88
Do molecular solids conduct electricity?
No
89
Ionic solids have what boiling and melting points?
High
90
When do ionic solids conduct electricity?
As a liquid or aq
91
Two covalent network solids are?
SiO2 (quartz) and diamonds
92
SiO2 (quartz) and diamonds have what melting and boiling points?
Very High
93
What are metallic bonds between?
Metals
94
Do metallic bonds conduct electricity?
Yes, always
95
What is a metallic bond's texture?
It varies
96
What breaks as a molecular solid boils or melts?
IMFs between the molecules
97
What is made when a smaller atoms fits in the gaps between the larger atoms in a metallic crystal?
Interstitial alloy
98
What is made when the radii of the metals are similar in size are substituted into the crystal lattice?
Substitutional alloy
