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Chemistry Semester 1 Final Flashcards | StudBud
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Chemistry Semester 1 Final
Chemistry Semester 1 Final
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Review for the semester 1 final of general Chemistry
Flashcards
40 cards
F
Practice quiz
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Host live
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Questions
40
Answers
1
Oxygen normally will make ___ covalent bonds.
2
3
4
1
2
An anion has ___ charge
Positive
Neutral
Negative
No Charge
3
Which of the following is a nonmetal
Y
Na
Pu
Cl
4
When writing electron configurations, what sublevel fills after the 5s sublevel
5p
5d
4d
3f
5
Which quantum number describes the shape of electron orbit
Sublevel
Energy level
Orbital
Spin
6
Why can't you use Celsius in gas law calculations?
Kelvin has an arbitrary zero point
It is impossible to convert between celsius and kelvin
it only works in farenheit
Celsius has an arbitrary zero point
7
Which quantum number describes the distance from the nucleus?
Orbital
Sublevel
Spin
Energy Level
8
A bond between a metal and a nonmetal is a/an___ bond
Metallic
Ionic
Hydrogen
Covalent
9
How many atoms are in 2 Moles of Carbon?
1.204 x 1024
6.022 x 1023
24.02
12.01
10
What is Mr. Shelby's wife's name?
Erica
Maryah
Paige
Jill
11
Which of the following is a pure substance?
Water
Steel
Iron
Cool Aid
12
Which of the following is Sodium Hydroxide?
SoOh
Na(OH)2
Na2(OH)3
NaOH
13
Light behaves as a ____
Kook
Particle
Wave
Brah
14
Which of the following will have similar properties to Barium?
Radon
Calcium
Radium
Cesium
15
Which of the following is a homogenous mixture?
Bubbles in Water
Salt and Sand
Chex Mix
Air
16
The electron geometry of water is ...
Tetrahedral
Bent
Linear
Trigonal Planar
17
What is the strongest intermolecular force
Dipole-dipole interaction
Hydrogen bonds
Ionic Bonds
Dispersion forces
18
How many valence electrons does Boron Have?
3
2
7
8
19
Metals always form ___
Anions
Cations
Legumes
Isomers
20
Which of the following causes dispersion forces?
Random Chance
Electron Symmetry
Evil Sprites
Temporary Dipoles
21
How many mm are in one cm
100
1000
10
1
22
Pressure and volume are
Directly Correlated
Dependent on other variables and cannot e used to predict.
Inversely Correlated
Unrelated
23
The maximum number of electrons in a valence energy level is ___
14 electrons
8 electrons
2 electrons
6 electrons
24
What is the weakest intermolecular force
Ionic Bonds
Hydrogen Bonds
Dispersion Forces
Dipole-dipole interactions
25
Which of the following is not a molecule
BaCl2
CCl4
CH4
H2O
26
Which of the following has the highest electronegativity
Sulfur
Oxygen
Cesium
Nitrogen
27
What is the strongest intermolecular force that C
5
H
12
experiences?
Dispersion Forces
Hydrogen Bonds
Dipole-dipole interactions
Ionic Bonds
28
How many sig figs does the following number have? 0.040
1
2
3
4
29
What is the correct answer to the following math problem: 5.50+4.50
10
1 x 101
10.00
10.0
30
Which of the following is a false assumption we make about ideal gases?
Gas particles are in constant motion
Gas particles experience no intermolecular attractions
Gases are compressible
Gas particles have no volume
31
Which of the following is not a chemical change?
Burning Coal
Cooking an egg
Rusting
Dissolving sugar in water
32
Which of the following is evidence for a permanent chemical change?
Release or absorption of heat/light
Formation of a gas (bubbles)
Permanent color change
Formation of a precipitate.
33
What are the units for molar mass?
Grams
Mass/Volume
Moles
Grams/Mole
34
According to VSEPR Theory ____
Electrons want to be as far apart as possible
Ionic compounds are always polar
Pressure and volume are inversely related
Electrons are attracted to protons
35
The shape of CH
4
is ....
Trigonal Pyramidal
Bent
Linear
Tetrahedral
36
An isotope is a form of an element that has a different number of _____
Neutrons
Electrons
Protons
Positrons
37
What is a mole in chemistry
A small furry, burrowing animal
A spy
6.022 x 1023
A birth mark
38
As wavelength increases, Frequency ____
Increases
These two both depend on other variables.
Decreases
Does not change
39
What happens at absolute zero?
Water freezes
There is no kinetic energy
Time stops
We don't know
40
When finding the empirical formula from the mass percent of a compound. What is the 2nd step?
If you get a fraction, multiply to make it a whole number.
Assume 100g sample
Divide by the smallest number
Convert to Moles
