Study Guide: Accel Chemistry Semester 1
How many significant figures do each of the following measured numbers
have, and to what precision have they been measured?
Example: 90 grams has one significant figure and is precise to the nearest ten grams.
1) 1234 liters
6) 9010 grams
2) 3010 grams
7) 3.4 x 103 meters
3) 890 degrees
8) 3.40 x 103 meters
4) 9010.0 grams
9) 0.0023 grams
5) 9010. grams
10) 1.0023 grams
Solve the following mathematical problems such that the answers have the
correct number of significant figures:
1) 334.54 grams + 198 grams =
4) 0.0010 meters – 0.11 meters =
2) 34.1 grams / 1.1 mL =
5) 349 cm + 1.10 cm + 100 cm =
3) 2.11 x 103 joules / 34 seconds =
6) 450 meters / 114 seconds =
Convert the following numbers into
scientific notation:
Convert the following numbers into
standard notation:
1) 3,750
5) 2.30 x 104
2) 0.00013
6) 1.76 x 10-3
3) 110,000
7) 1.901 x 107
4) 0.0100
8) 8.65 x 10-7
Density = Mass/Volume
What are the differences between an element, a compound, a homogeneous mixture, and
a heterogeneous mixture? Give an example of each.
How do chemical properties differ from physical properties? How do chemical changes
differ from physical properties? Give an example of each.
What is the law of conservation of mass?
In what ways was the Greek model of the atom the same as that of Dalton's model?
In what ways was the Greek model of the atom different than that of Dalton's model?
What did Thomson’s cathode ray experiment prove?
What was Rutherford’s experiment, and what did he find out about the atom?
What was Niels Bohr’s model of atom?
What is quantum mechanics?
Explain how and why only certain colors of light are given off when an atom is heated.
How many protons, neutrons, and electrons does an atom of
Protons: _____
Neutrons: _____
261Rf
have? (3 pt)
Electrons: _____
Forming ions: what happens when an element loses an electron? What happens when an
element gains an electron?
What is the general equation for determining the average atomic mass of an element from
its isotopic abundances? What does this calculation mean?
EMR Problems: useful equations
λν = c
c = 3.00 x
E = hν
108
m/s
H = 6.626 x 10-34 J x s
1. Ultraviolet radiation has a frequency of 6.8 × 1015 1/s. Calculate the energy, in joules, of
the photon.
2. A sodium vapor lamp emits light photons with a wavelength of 5.89 × 10-7 m. What is
the energy of these photons?
3. Find the energy in kJ for an x-ray photon with a frequency of 2.4 × 10181/s.
4. A ruby laser produces red light that has a wavelength of 500 nm. Calculate its energy
in joules.
5. What is the frequency of UV light that has an energy of 2.39 × 10-18J?
6. What is the wavelength and frequency of photons with an energy of 1.4 × 10-21 J?
Atomic & Molecular
Structure
Atomic number
1. What is atomic number?
2. What is atomic number for the following
elements?
Cr
Iron
Atomic structure
1. Draw an atomic model of
Carbon-13.
In the drawing include the following:
 Location of nucleus & electron cloud.
 Location of 3 subatomic particles.
 Amount of each subatomic particles.
 A note where most of the atom’s
mass is found.
Carbon
C
3. How does atomic number change moving left to right across the periodic table?
Atomic Weight (Atomic Mass)
4. What is the atomic mass for the following elements?
V
Oxygen
Organization of the Periodic Table
1. Identify on the periodic table below
Beryllium
Mn
the location of
The 3 different types of elements.
5. It was found that the periodic table was
organized by increasing atomic number
rather than mass. Give an example of a
pair of elements where one element has a
larger atomic number but a smaller
atomic mass.
6. Identify the letters in the following periodic
square:
2. Where are groups on the periodic
table?
3. Where are periods on the periodic
table?
Periodicity (periodic trends)
7. Atomic Radius
 Which element has the largest atomic radius?

Which element has the smallest atomic radius?
8. Ionization energy
 What is Ionization Energy?

Which element has the largest ionization energy?

Which element has the lowest ionization energy?

Why does ionization energy decrease moving down a group?
9. Electronegativity
 What is Electronegativity?

Which element has the largest electronegativity?

Which element has the lowest electronegativity?

Why do Noble Gases tend to have no electronegativity?
Valence electrons
10. Why are alkali metals so reactive?
11. Why are halogens so reactive?
12. Identify the amount of valence electrons in each of
the following:
Na
Phosphorus
Ba
How many of magnesium
atom’s 12 electrons are
valence electrons? Circle
those electrons.
Helium