Download Name: Date: Chemistry Enriched Per. ______ Midterm Review

Name: __________________________________________
Date: _________________________
Chemistry Enriched
Midterm Review Sheet
Per. ________
Measurement & Problem Solving:

Determine the number of significant figures
o
0.0101 ____________
500.025 ________________
34.200_______________

Convert 55 cm to km:

Convert 44.5 grams to mg:

Express the answer with the correct number of significant figures.
33.4 + 2.45 + 0.2788 =
44.7 x 0.27 =

What is the density of Al if it has a mass of 54.0 g and a volume of 21 ml?

What is the volume of copper that has a mass of 50.0 g and a density of 7.9 g/ml?

What are the SI units of count, volume, mass, temperature, length, & energy?
Properties of Matter:

Describe the difference between pure elements, pure compounds, and mixtures.
Elements

Pure Compounds
Mixtures
Give at least 2 examples each, in your home,
o Elements - ________________________________________________________________________
o Compounds - _____________________________________________________________________
o homogeneous mixtures - _______________________________________________________
o heterogeneous mixtures - ______________________________________________________
o alloys-_____________________________________________________________________________

A tree grows in the woods…It is then chopped down and cut into firewood. You
split the logs and let them “season” (dry out) for at least 6 months. You then
burn the firewood in your highly efficient, “clean” burning wood stove. Describe
the chemical and physical processes taking place…and describe how you know
the difference…

What is the difference between a heterogeneous mixture and a homogeneous
solution?

Know the difference between filtration, crystallization, and distillation.
Filtration
Crystallization
Distillation

How would you go about separating a mixture of salt, sand, and water?

Describe the packing and motion of particles in solids, liquids, and gases:
Solids
Liquids
Gases
Arrangement of
particles
Volume
Shape

Describe a reversible physical process and an irreversible physical process:

State the law of conservation of matter:

Apply the law of conservation of matter: If 18 grams of water is decomposed
and 16 grams of oxygen are produced, how many grams of hydrogen were
produced?
The Atom

Can you name Dalton’s 4 main points of his Atomic Theory?
o
o
o
o

Describe both Thomson’s cathode ray experiment and Rutherford’s gold foil
experiment and how this changed our understanding of the atom. What models
of the atom did each propose as a result of their experiments?
Thomson’s Cathode Ray Experiment
Rutherford’s Gold Foil Experiment

What does the atomic number stand for on the Periodic Table?

Describe both the charge and relative atomic masses of each of the 3 primary
sub-atomic particles.
o
o
o

Initially, hydrogen was the “standard” all atoms were compared to…today, all
atoms are compared to which atom?

Using the Periodic Table, describe the number of protons, electrons and average
number of neutrons in Boron, Aluminum, and Gold.
# Protons
# Electrons
Average # of
Neutrons
Boron
Aluminum
Gold

Atomic masses are not whole numbers due to isotopes, what are isotopes?

Chlorine consist of 2 isotopes, Cl-35 at 75.77% abundance and Cl-37 at 24.23%
abundance. What is the average atomic mass of chlorine?
Electrons in Atoms

Describe the Bohr model of the hydrogen atom. What is his model compared to?
Include a drawing.

What is Bohr’s explanation on how an atom’s electrons emit light?

What is a quanta? How can you find the energy of a quantum?

Compare and contrast ground and excited state.

How does wavelength relate to frequency of light?

If a radio broadcasts at a frequency of 101.5 MHz, what is the wavelength of the
radio signal?

What is the energy of a photon that has a frequency of 98.7 MHz?

Describe Schrodinger’s quantum mechanical model of electron orbitals.

Apply the Aufbau principle, Hund’s rule, and the Pauli Exclusion Principle to
write the electron configurations for Na, O, Ni, & Sn.
Na
O
Ni
Sn

Where is the “s” block, “p” block, “d” block, and “f” block on the periodic table?

How does the Periodic Table inform you of electron configurations?
The Periodic Table

Describe Mendeleev’s Periodic Table and how he organized it.

Why did Mendeleev leave blanks in his Periodic Table? What did the blanks
represent?

How was Mendeleev able to accurately predict many of the properties of
Germanium and Gallium (elements not yet discovered)?

Why did Moseley change the order of the elements from atomic mass to atomic
number? (And, why didn’t Mendeleev think of this?)

What is the Periodic Law?

Elements were grouped together by similar chemical properties. What gives
these elements similar chemical properties?

The vast majority of elements are good conductors of electricity, shiny, and
malleable…as a broad class they are called what and where are they located?

Silicon is a semiconductor sometimes behaving like a metal and sometimes like a
nonmetal. What type of element is silicon?

Where are the halogens, noble gases, alkali metals, and alkaline earth metals
found? What do you know about these groups (reactivity, valence electrons,
properties)?
Location
Halogens
Noble Gases
Alkali Metals
AlkalineEarth Metals
Reactivity
Valence
Electrons
Properties

What are the “d” block of metals called?
Nuclear Chemistry

Describe at least 3 types of nuclear decay.
o
o
o

Be able to write balanced nuclear equations based on alpha decay or beta
decay.
o Alpha-Decay Example-
o
Beta-Decay Example-

How can you utilize the concept of half-life to determine the age of a fossil or
to determine how much radioactive sample is left after a given amount of
time?

Calculate the age of a fossil if 12.5 mg of C-14 remains and the original fossil
contained 100 mg of C-14. The half-life of C-14 is 5,730 years.

I-131 has a half-life of approximately 8 days. How much of a 50 mg sample
remains after 48 days?

What is nuclear fission?

What is nuclear fusion?

What process does the sun use to produce its energy?

What process do nuclear power plants use to produce electricity?
The Mole

Utilize the mole concept to determine number of atoms/molecules given the
mass of a substance (and vice-versa).
o How many grams Magnesium in 2.5 moles Mg?
o How many moles Chlorine in 15.0 grams Cl?
o How many atoms in 10.0 grams of Carbon?
o How many grams NaCl in 3.01 x 1022 formula units of NaCl?

Be able to determine the % composition of elements in any compound. What
is the % composition of each element in Na3PO4?
o Na
o P
o O

What is an empirical formula?

What is the empirical formula of the following molecular formulas?
o C6H12O6 –

o C4H10 –
Be able to determine the empirical formula of a compound given either %
composition or mass of each element in the compound.
o What is the empirical formula of a compound that consists of 18.8%
Li, 16.6% C, and 64.9% O?
o What is the empirical formula of a compound that consists of 52.9% Al
and 47.1% O?

What is the molecular formula of a compound that has an empirical formula
of C3H6N2 and a molecular molar mass of 210 g/mol?