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2024 Fall Honors Chemistry 1 Exam Review Flashcards | StudBud
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2024 Fall Honors Chemistry 1 Exam Review
2024 Fall Honors Chemistry 1 Exam Review
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1
The lowest allowable energy state is called...
orbital
quantum
photon
ground state
2
A hydrate that has had all its water removed through heating would be called...
dehydrous
amphoteric
anhydrous
supernatant
3
What are isotopes?
elements with same # of protons but different # of neutrons
elements with same # of protons but different # of electrons
elements with same # of neutrons but different # of protons
elements with same # of electrons but different # of protons
4
What is the name for K
2
CrO
4
?
potassium chromate
potassium dichromate
potassium (I) dichromate
potassium (I) chromate
5
What two subatomic particles are very similar in mass?
protons and electrons
electrons and neutrons
protons and neutrons
None of the particles are similar in size
6
How many neutrons does cobalt - 56 have?
56 neutrons
29 neutrons
27 neutrons
30 neutrons
7
Who designed the original Periodic Table?
Dalton
Mendeleev
Meyer
J.J. Thomson
8
Which of the following describes water?
solution
homogeneous mixture
heterogenous mixture
compound
9
When preparing an acid solution...
add water to acid quickly
add acid to water quickly
add water to acid slowly
add acid to water slowly
10
Who developed the modern atomic theory?
Dalton
J.J. Thomson
Milikan
Rutherford
11
What types of orbitals are found in n=2?
only s, p, and d
only s
only s and p
s, p, d, and f
12
Which type of intermolecular force occurs between polar molecules?
hydrogen bonding
diffraction forces
dispersion forces
dipole-dipole forces
13
During the hydrogen lab, what two substances reacted to form hydrogen gas?
oxygen and sulfuric acid
oxygen and hydrochloric acid
zinc and hydrochloric acid
zinc and sulfuric acid
14
Which of the following does NOT explain why atomic radii get larger as you move down a group?
Another energy level or ring is added.
There are less shielding electrons.
Electrons in the atom are pushed to higher energy levels.
There are more electrons in the atom.
15
How many total orbitals are found in the 3rd principal energy level, n = 3?
9
16
3
4
16
Which best describes wood burning?
chemical property
physical extensive property
physical property
physical intensive property
17
What is group 7a called on the periodic table?
halogens
rare earth metals
noble gases
alkali metals
18
What is the name of Li
2
O
2
?
lithium peroxide
lithium (II) oxide
lithium (I) oxide
lithium (I) peroxide
19
Which principal quantum number has the most energy?
n = 2
n = 1
n = 3
n = 4
20
When an oxide like Ba(ClO
3
)
2
is heated, what is released?
Cl2
oxygen
water
BaCl2
21
Who was the Greek philosopher that originally came up with the idea of atoms?
Rutherford
Democritus
Milikan
J.J. Thomson
22
Which element in the d block has multiple charges and thus needs a roman numeral?
silver
zinc
cobalt
cadmium
23
Which of the following describes an atom?
macroscopic
scanning tunneling microscope
submicroscopic
light microscope
24
How many oxygen atoms are in the following formula: Ca
3
(PO
4
)
2
?
13
8
4
6
25
Which best describes melting point?
physical extensive property
chemical property
physical intensive property
physical property
26
Name the orbital if n=3 and l = 1.
2s
3d
3p
3s
27
Which separation technique would best separate two liquids from each other?
filtration
distillation
crystallization
28
How many significant figures does the number 0.05320 have?
5
3
4
6
29
Which best describes a theory?
something that can't be modified
a statement that explains what happens
A statement that has no exceptions
explanation supported by many experiments
30
Which of the following statements about atomic orbitals is NOT correct?
Orbitals are probable locations.
Orbitals come in different shapes.
Orbitals are where electrons can be found.
Bohr came up with the idea of orbitals.
31
Which element below would most likely lose 2 electrons to form a bond?
Barium
Carbon
Iodine
Rubidium
32
What is the name of SnO?
tin oxide
tin (II) oxide
tin (II) peroxide
tin peroxide
33
How do you find the number of neutrons in an isotope?
atomic number - protons = neutrons
neutrons = mass number
mass number - atomic number = neutrons
neutrons = atomic number
34
What is the SI base unit for mass, temperature, and amount?
kg, degrees F, mole
kg, K, mole
g, degrees F, mole
g, K, mole
35
Which of the following properties is NOT a property of ionic compounds?
electrical conductors
high melting and boiling points
brittle
softer solids
36
In hydrogen bonding, a hydrogen of one dipole could be attracted to all of the below except...
Fluorine
Nitrogen
Phosphorus
Oxygen
37
What law states that matter is not created nor destroyed only changed in form?
Law of Definite Proportions
Law of Conservation of Mass
Law of Multiple Proportions
Law of Gravity
38
What is the name of HCN?
cyanic acid
cyanous acid
hydrocyanic acid
cyanide acid
39
What does the term vapor mean?
a gas which is a solid at room temperature
a gas at room temperature
a gas which is a liquid or solid at room temperature
a gas which is a liquid at room temperature
40
Which group of elements has the most negative electron affinities?
noble gases
halogens
alkali metals
transition metals
41
Which is an example of a physical change?
decomposing tree
melting ice cube
burning candle
rusting car
42
The mixing of one s and one p orbital creates which of the following?
1 sp orbital
2 sp2 orbitals
2 sp orbitals
1 sp2 orbital
43
Which of the following groups is least reactive?
Alkaline Earth Metals
Transition Metals
Halogens
Alkali Metals
44
Earth's gravitational pull on an object is...
volume
density
mass
weight
45
Which of the following indicates when ionic compounds are NOT good conductors?
ionic compounds are liquids
ionic compounds are solids
ionic compounds are dissolved
ionic compounds are melted
46
Atomic radii _______________ across a period.
decreases
stays constant
increases
47
The energy needed to remove an electron is called...
lattice energy
electronegativity
ionization energy
electron affinity
48
Who discovered the electron?
J.J. Thomson
Milikan
Dalton
Rutherford
49
The quantum of light energy released when electrons move within an atom?
photon
orbital
ground state
quantum
50
From the options below, which group has the highest ionization energy and which has the lowest?
high - Group 7A low - Group 2A
high - Group 2A low - Group 7A
high - Group 8A low - Group 1A
high - Group 1A low - Group 8A
51
What is the formula for aluminum phosphate?
Al2(PO4)3
Al3(PO4)2
AlPO4
Al3(PO4)3
52
What is the formula for hydrosulfuric acid?
H2SO
H2S
H2SO4
H2SO3
53
Which scientist said that electrons travel in exact locations called orbits?
Schrodinger
Bohr
Heisenberg
De Brogile
54
What is the formula for Cl
2
O
7
?
dichloride heptoxide
dichlorine hexoxide
dichloride hexoxide
dichlorine heptoxide
55
Which of the following is NOT a homogeneous mixture?
solution
chunky peanut butter
brass
salt water
56
What color of visible light possesses the least energy?
yellow
blue
violet
red
57
If the electronegative difference is 1.30, what type of bond is it?
polar covalent
ionic
non-polar covalent
metallic
58
Which of the following is always true for an electron in a s orbital.
the value of ms is 1.
the value of ml is 0.
the value of n must be 3.
the value of l is 2.
59
Who discovered the nucleus through the gold foil experiment?
J.J. Thomson
Democritus
Dalton
Rutherford
60
The 4 quantum numbers 2, 1, 1, 1/2 describe an electron in an unfilled sublevel of...
N
P
Mg
Be
