Download CHEMISTRY FALL FINAL PRACTICE 2016

Review Practice for Chemistry I Advanced
freezing point _____
Measurements:
1.
Identify as quantitative or qualitative data:
red _______
three meters _______
3.
A student measures the volume of water to be
4.5 mL, 5.9 mL and 3.2 mL. If the water’s volume is
actually 2.5 mL, how would you describe the
student’s measurements in terms of accuracy and
precision?
How many significant digits does each of the
following have:
45000 ____ 0.00320 ______
5.
Calculate the following using proper significant
digits:
4.5 + 7.87 = ______ 6.53 x 2.345 _________
6.
What is the volume of a rectangle with the
dimensions of 5.78 cm, 2.09 cm and 2.3 cm? ______
7.
Write the measurements in scientific notation:
789 000 km =______________
0.00089 mm = _______________
What is the mass if the density is 1.87 g/cm3
and a volume of 4.5 cm3?
What is the volume if the density is
0.76 g/ml and the mass is 6.7 grams?
b.
Why does an object sink?
c.
If a cube has one side measuring 2.0 cm3
and it has a mass of 30.0 g, what is its
density?
d.
Aluminum has a density of 2.70 g/cm3 and
iron has a density of 7.87 g/cm3. A
substance has a mass of 45 g and a volume
of 16.7 cm3, what is the substance likely to
be?
e.
Look
at the
Y
picture.
The
glass is filled with three different colorless
liquids. Decide which letter represents the
most dense object. How do you know?
f.
If a piece of wood with a density of 10.00
g/cm3 is cut in half, what is the density of
each piece of wood?
Why?
Write the following in standard form:
5.6 x 10-2 cm ________________
2.34 x 105 m = ______________
9.
What is the density of a substance with a
mass of 16.5 grams and a volume of 3.6
mL?
Round 54 6378 to three significant figures
_________________
4.
8.
volume ____
3.
a.
2.
odor _____
Do the following calculations to the correct number
of significant digits.
5.6 x 102 X 2.34 x 105 = ________________
Be able to use dimensional analysis/factor label to
make conversions.
56 g = _____________________ mg
2.6 days = _____________________ s
10. If you wanted to get the density of a block of wood,
what tools would you need?
4.
Identify as a physical and chemical change:
Evaporation of alcohol ____ tarnishing silver ____
Leaves changing colors __ wood decays ____
Freezing water ___ biting a cookie ____
Combustion of oil ____ nail rusting _____
5.
Describe the difference between a mixture and a
compound.
If you wanted to get the density of a rock, what tools
would you need?
Matter and Change
1.
Identify as a physical or chemical property
Flammability ____ malleability ____ viscosity _____
2.
Identify as an intensive and extensive physical property.
Red color ____
mass ____
density ____
X
Give three examples of each.
e.
6.
A clear liquid evaporates and leaves a yellow solid. The
original liquid was what type of matter?
Explain.
f.
What is the mass number of the most
common isotope of cobalt. _________
Write the nuclear notation for the most
common isotope of chromium.
6.
If a substance always has one atom of sulfur and three
atoms of oxygen, it is an example of what type of matter?
Explain.
Identify the following as a pure substance (element or
compound) or a mixture (homogeneous and
heterogeneous).
oxygen ___
dirt ____ sodium chloride ___
sugar water ___ muddy water ___
iron ____
7.
What is the smallest part of an element that has all of the
properties of the element? __________
8.
Describe particles in the diagrams as being: mixtures,
pure substances, compounds, and elements.

  
  

Use the periodic table to find the following
information concerning the element with 15 protons:
a. Get the atomic number _________
b. Identify the element __________________
c. Find the mass number of the most common
isotope of an element _________
d. Get how many neutrons the most common
isotope has _________
e. How many valence electrons an element has
_________
f. What is its charge/oxidation number for the
atom _________
g. Know what ion is forms/write the ion _______
h. The name of the ion __________________
7. Describe the three subatomic particles in the atom?
Subatomic
charge
location
particle



8.
Atomic Structure:
1.
2.
3.
4.
5.
What is the charge on the nucleus? ____________
What is inside the nucleus? ____________
What is the charge on the electron cloud? ____________
What is inside the electron cloud? ____________
Of the nucleus and the electron cloud, which is most
dense? ____________
If an atom is electrically neutral, what is true about its
particles? __________________________________________________
Define mass number.
a.
How is the mass number calculated?
How do you find the number of neutrons an atom has?
______________________________________________________________
a.
Define isotope:
b.
c.
If two atoms are the same element, what
must be the same? _______________________
The number written after the name of an
isotope (Ex. Cabon-12), represents what?
_________________________
d.
80Br
35
Identify the following:
i.
ii.
iii.
iv.
Atomic number _________
Number of protons_________
Number of neutrons_________
Number of electrons _________
9.
Identify the protons, neutrons, and
electrons
b. What is this atom/element _____________
c. What is it’s mass number? _____________
There are four naturally occurring isotopes of the
make-believe element Katrayden (Ka). Based on the
following, what is the average atomic mass?
172
169
Ka 22.63 %
Ka 6.42%
171
Ka 12.52%
170
Ka 58.43%
Name an element in the same group as oxygen. ______
Electron Arrangement and Periodic Table:
1.
Name the four sublevels and identify how many
orbitals are in each.
11. Name an element with similar properties to
magnesium. ______ How do you know? _________________
2.
How many electrons can occupy the s orbital? ____
p orbital? ____
How many electrons are needed to fill the 2nd energy
level? ________
Identify this element: 1s2 2s2
How do you know?
12. Which has the smallest atomic radius: Mg or S
Why?
3.
4.
5.
Write the electron configuration for:
Si
13. Repeat #12, but with which has the largest ionization
energy. Mg or S
Why/how do you know?
Mg or Ca
Why/how do you know?
Ca
Fe
6.
Which has the smallest atomic radius: Mg or Ca
Why?
14. Which element the largest electronegativity. ______
15. How many valance electrons does each group 2A
have?_______ group 6A? _____
Write the Aufbau diagram for:
Li
Bonding
Cl
1.
Identify the following as ionic or covalent:
a. HCl ____
d. NO _____
b. MgCl2 ____
e. CCl4 ____
c. SF2 ____
f. Na3P ____
2.
How many bonds do each of the following tend to
form? C ___
O ____
N ___
H_____
3.
List four properties of covalent compounds:
4.
List four properties of ionic compounds:
5.
List the seven diatomic molecules and indicate the
number of bonds between them.
6.
Draw the following Lewis structures and identify
their shape.
CF4
CO2
Mg
7.
Write the noble gas notation for:
S
K
Fe
8.
How many electrons are in the highest energy level of:
1s2 2s22p6 3s2 3p64s23d2 _____
Identify this element ___________________
9.
Describe each of the following in terms of valence
electrons, block on periodic table, and outer electron
configuration: alkali family, alkaline-earth metals,
halogens and the noble gases by completing the table:
Alkali
Alkalineearth
halogens
H2O
NH3
PH3
CBr3F
Noble
gases
Valence
electrons
Block on
periodic table
Outer electron
configuration
10. Name an element in the same period as lithium. ______
Mole …is back
1. How many atoms are in 1 mol iron? ________________
Lithium? ________________
2. What is the molar mass of manganese? ________
Oxygen? ________ Gold? ________
3. How many moles of magnesium are in 35.6 g of
magnesium?
How many moles of lithium are in 75.89 g of lithium?
How many atoms are in 6.53 moles of carbon?
How many atoms are in 13.8 moles of Chromium?
Identify the following pieces of lab equipment and what
they are used for.