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Final BAT
Name: ___________________________________________ Date: ____________________ Period: ___
The final will be comprehensive, covering chapters 1-18, with the focus on chapters 10 – 18. The
following questions will be what you have to Be Able To do for the final. Complete the following
questions. Where it says important topics, you do not have to write anything, just study those topics in
those chapters.
Chapter 1
Important topics: homogeneous mixture, heterogeneous mixture
1. Place a X in the box to indicate whether the following substance is an element or a compound
Substance
H2
MgCl2
Ne
Cl2
NaC2H3O2
Element
Compound
2. Place a X in the box to indicate whether the following element is a metal, nonmetal, or metalloid
Element
N2
Ca
Si
Co
Metal
Nonmetal
Metalloid
Chapter 2
Important topics: significant figures, directly proportional, inversely proportional
3. A chunk of wood has a mass of 258g and occupies 122 cm 3. What is the density of this wood?
4. The density of water is roughly 1.0g/mL at room temperature. Would the chunk of wood float or
sink in water? Why?
5. Under certain conditions, oxygen gas (O2) has a density of 0.00134 g/mL. What is the volume
occupied by 250.0 g of O2 under the same conditions?
Chapter 3
Final BAT
Name: ___________________________________________ Date: ____________________ Period: ___
Important topics: law of conservation of mass, definition of atomic mass, definition of isotope,
definition of ions
6. Fill in the table below to determine the number of protons, neutrons, and electrons.
Nuclear Symbol
Protons
Neutrons
Electrons
26
30
23
7. Fill in the table below
Element
Number of valence
electrons
Ionic charge
K
O
Ca
F
N
Al
8.
Write the electron configuration for
a. Na
b. Mg+2
c. Cl-1
9. Fill in the electrons in the orbital diagram below for sulfur
Final BAT
Name: ___________________________________________ Date: ____________________ Period: ___
Chapter 5
Important ideas: shielding, nuclear charge, definition of ionization energy, definition of electronegativity
10. Fill in the table below to identify the proper element
Description
Element symbol
Alkali metal in period 3
Halogen in period 2
Any transition metal in period 5
Noble gas in period 4
Alkaline earth metal in period 6
11. Which element has…
a. Higher atomic radius: F or I
b. Lower atomic radius: Na or Cl
c. Higher electronegativity: C or O
d. Lower electronegativity: I or F
Chapter 6
Important topics: octet rule, intermolecular forces (hydrogen bonding, dipole, dispersion)
12. Place a X in the box to indicate whether the following compound is ionic or covalent
Compound
Ionic
Covalent
CaCl2
NO2
AlBr3
CH4
NH4Cl
13. Draw the Lewis structure for CF4
14. Write the shape notation and determine the shape of the compound drawn above
15. Is the compound drawn above is polar or nonpolar?
16. What type of intermolecular force does a sample of CF4 have?
17. Draw the Lewis structure for the compound formed between Mg and Cl
Final BAT
Name: ___________________________________________ Date: ____________________ Period: ___
Chapter 7
Important topics: naming rules for ionic compounds, covalent compounds, acids
18. Give the formulas for the following compounds
a. iodine pentafluoride _____________________________
b. sulfurous acid __________________________________
c. aluminum sulfide _______________________________
d. acetic acid _____________________________________
e. cobalt (III) carbonate ____________________________
f.
dinitrogen trioxide ________________________________
19. Give the names for the following compounds
g. P4S5 __________________________________
h. Mg(CH3COO)2 ___________________________________
i.
H2CO3 __________________________________
j.
Si2Br6 __________________________________
k. H3P _____________________________________
l.
Ni(OH)2 ________________________________________
Chapter 8
Important topics: 5 types of reactions
20. Write the balanced chemical reaction with the states of matter given the following descriptions
a. Ethane (C2H6) burns
Final BAT
Name: ___________________________________________ Date: ____________________ Period: ___
b. Potassium chloride reacts
c. Calcium and nitrogen react
d. Magnesium metal is added to a solution of copper (II) chloride
e. Solutions of barium nitrate and sodium sulfate are mixed together
Chapter 9
Important topics: molar mass, mole ratio, theoretical yield, percent yield, limiting reactant
1. For the following reaction:
2 Al + 3 CuCl2 → 3 Cu + 2 AlCl3
a.
How many moles of aluminum are needed to completely
react with 0.00789 moles of copper (II) chloride?
b.
How many grams of aluminum are needed to completely
react with 0.004365 moles of copper (II) chloride?
c.
How many moles of copper (II) chloride are needed to
completely react with 0.25 grams of aluminum?
Final BAT
Name: ___________________________________________ Date: ____________________ Period: ___
d.
How many grams of copper (II) chloride are needed to
completely react with 0.15 grams of aluminum?
e.
Which reactant is the limiting reactant if there are only 1.254
grams of aluminum and 6.348 grams of copper (II) chloride available for this reaction?
f.
What is the theoretical yield of copper when 1.254 grams of
aluminum and 6.348 grams of copper (II) chloride react?
g. When this reaction was carried out in the lab, 3.487 grams of product was obtained.
What is the percent yield of this reaction?
Chapter 10
Important topics: kinetic molecular theory, gas laws – Boyle, Charles, Gay-Lussac,
combined, Dalton
If the temperature is held constant in the diagram above, name the gas law being
illustrated, and describe how the variables change.
Final BAT
Name: ___________________________________________ Date: ____________________ Period: ___
In the above container, with a fixed volume, the temperature is increased from the first picture to the
2nd.
1. Describe the change in kinetic energy of the particles
2. Name the gas law and describe how another variable, in addition to temperature will change.
The temperature of a 3.00 L sample of gas is changed from 5 to 25 oC. what will the volume of gas be at
the new temperature if pressure is held constant?
A student collects 350 mL of oxygen gas at a temperature of 24 oC and a pressure of 0.85 atm. How
many moles of oxygen did the student collect?
A gas occupies 13 liters at a pressure of 50 mm Hg. What is the volume when the pressure is increased
to 75 mm Hg?
600.0 mL of air is at 20 oC. what is the volume at 60.0 oC?
Final BAT
Name: ___________________________________________ Date: ____________________ Period: ___
A sample of oxygen is collected in a 175 mL container over water at 35 oC when the barometric pressure
reading is 742.0 torr. What is the partial pressure of the dry gas?
If a mixture of gases contains 3 gases - carbon dioxide with a partial pressure of 0.285 torr and nitrogen
with a partial pressure of 593.525 torr and oxygen at partial pressure = ? find the partial pressure of
oxygen.
What is the density of silicon tetraflouride gas at 68 oC and pressure = 135 kPa?
A gas sample at 47 oC and 1.03 atm occupies a volume of 2.2 L what volume would this gas occupy at
107 oC and 0.789 atm?
What is the mass of 85.0 L of NO2 at STP?
How many grams of calcium carbonate is needed to form 2.5 L of CO2 when calcium carbonate is
decomposed (see chapter 8 decompostion if you need to figure out equation)?
Chapter 12
Final BAT
Name: ___________________________________________ Date: ____________________ Period: ___
Important topics: Particle behavior in liquids and solids, phase changes, molar heat of fusion, molar
heat of vaporization, phase diagrams, equilibrium vapor pressure
Describe the change in the particles and indicate if heat is added or removed when:
a)
b)
c)
d)
A liquid changes to a vapor
A liquid changes to a solid
A vapor changes to a liquid
Solid CO2 sublimes
How is boiling different from evaporation?
During the boiling process – describe what is happening to the particles and the temperature.
Explain why glycerol boils at a higher temperature than water (in terms of the attractive forces
between molecules)
At a given temperature, different liquids have different equilibrium vapor pressures. Explain why
this is true (in terms of attractive forces between molecules).