Name____________________
CHEMISTRY MID-TERM REVIEW
CHAPTERS 1 AND 2
TERMS AND CONCEPTS:
Atom
pure substance
mixture
element
Compound
homogeneous
heterogeneous
matter
Mass
volume
density
metric prefixes
Chemical change
physical change
scientific notation
scientific method
Hypothesis
theory
law
branches of chemistry
Accuracy
precision
law of conservation of energy types of research
Intensive property
extensive property
SKILLS/PROBLEM TYPES:
Metric conversions
Density
Significant figures/calculating with sig figs
Scientific notation
How to tell between physical and chemical changes
How to tell between pure substance, homogeneous, and heterogeneous mixtures
PRACTICE PROBLEMS:
1.
How many mL are equal to 550 cL?
2.
How many ng are equal to 5.5 x 10-6 hg?
3.
What is the density of a block of marble that occupies 310 cm3 and has a mass of 853 g?
4.
Diamond has a density of 3.26 g/cm3. What is the mass of a diamond that has a volume of
0.350 cm?
5.
What is the volume of a sample of liquid mercury that has a mass of 76.2 g given that the
density of mercury is 13.6 g/mL?
6.
How many significant figures are in each measurement?
a. 500 m _____________
c. 0.00005 m_______________
b. 0.0500 m ____________
d. 50 m ___________________
7.
Make the following calculation and report your answer to the correct number of significant
figures please.
a. 55.46 g - 28.9 g _________________________
b. 0.021 cm x 3.2 cm x 100.1 cm________________
c. 1.278 x 103 m2 / 1.4267 x 10 2 m_______________
8. Put each number in scientific notation please.
a. 0.005 _______________
b. 5 050 _________________
c. 0.00025 _________________
d. 5 200 000 ________________
Name________________
CHEMISTRY MID-TERM REVIEW
CHAPTERS 3, 4, and 5
TERMS AND CONCEPTS:
Law of definite proportions
Nucleus
Electron
Mass number
Orbital
Quantum numbers (4)
Pauli Exclusion Principle
Mendeleev
Group
Main-group elements
Lanthanides
Electronegativity
law of conservation of mass
proton
Rutherford
isotopes
ground state
Aufbau Principle
mole
Mosely
period
Group Names (1,2,17,18)
actinides
ionization energy
law of multiple proportions
neutron
atomic number
Dalton
excited state
Hund’s Rule
Avogadro’s number
periodic law
valence electrons
transition metals
alloy
atomic radius
SKILLS/PROBLEM TYPES:
Istopes
Molar conversions
Electron configurations
Periodic trends
PRACTICE PROBLEMS:
1. Give the number of protons, neutrons, and electrons in each isotope please:
a. Sodium-23
b. Mercury-201
c. Uranium-238
2.
How many grams of silver are in 0.45 moles of silver?
3.
How many moles of bromine are in 345 g of bromine?
4.
How many carbon atoms are in 45.9 grams of carbon?
5. Give the electron configuration for each element in “all three” notations please.
a. K
b. Bi
c. I
6. Circle the atom with the larger atomic radius please.
a. Ba
or
Ca
b. Ni
or
Pt
c. Cl
or
Al
7.
Circle the element with the higher ionization energy please.
a. Ba
or
Ca
b. Ni
or
Pt
c. Cl
or
Al
8.
Circle the element that is more electronegative please.
a. Ba
or
Ca
b. Ni
or
Pt
c. Cl
or
Al
Name___________________________
CHEMISTRY MID-TERM REVIEW
CHAPTERS 6 and 7.1
TERMS AND CONCEPTS:
Ion
polyatomic ion
Ionic bond
octet rule
Polar covalent
nonpolar covalent
Single bond
double bond
Resonance structure covalent prefixes
SKILLS/PROBLEM TYPES:
Know the polyatomic ions!!!!!!!!!!!!!!!!
Naming ionic compounds
Writing ionic formulas
Naming covalent compounds
Writing covalent formulas
Drawing Lewis structures for elements
Drawing Lewis structures for molecules
Assigning oxidation numbers
cation
covalent bond
bond length/energy
triple bond
charges for each group
anion
molecule
Lewis structure
VSEPR Theory
PRACTICE PROBLEMS:
1. Name the following ionic compounds assign oxidation numbers to each please.
CaCO3_________________________
Zn3(PO4)2______________________
Fe2O3__________________________
NaClO3_________________________
NH4NO3________________________
CuC2H3O2_______________________
2. Name the following covalent compounds please and assign oxidation numbers to each please.
NH3________________________________
SiO2________________________________
N2O5________________________________
PBr3_________________________________
C3H8_________________________________
SCl6__________________________________
3. Give the formula for each ionic compound please.
Lead (IV) chromate__________________________
Magnesium hydroxide________________________
Potassium nitrate____________________________
Calcium chlorate____________________________
Iron (II) chloride______________________________
Aluminum sulfide_____________________________
4.
Give the formula for each covalent compound please.
Carbon monoxide_______________________
Pentacarbon octahydride__________________
Carbon disulfide__________________________
Dinitrogen trioxide________________________
5. Decide if each is ionic or covalent and name appropriately please.
Si2O4__________________________________
Na2O__________________________________
Al2(SO4)3_______________________________
N2O6__________________________________
PbSO4__________________________________
6. Decide if each is ionic or covalent and write the correct formula please.
Aluminum hydroxide__________________________
Calcium carbonate____________________________
Sulfur trioxide_______________________________
Sodium phosphide____________________________
Hexacarbon decahydride_______________________
7. Draw a Lewis structure for each element please.
a. Li
b. I
c. He
8.
Draw Lewis structures for each compound please. Use resonance structures if applicable.
CO
CO2
NO3 1-
CH3I
C3H6
CO3 2-
Name_____________________
CHEMISTERY MID-TERM REVIEW
CHAPTERS 7 AND 8
TERMS AND CONCEPTS:
Average atomic mass
Molecular formula
Catalyst
Single replacement reaction
Coefficient
percent composition
reactants
synthesis reaction
double replacement reaction
empirical formula
products
decomposition reaction
combustion reaction
SKILLS/PROBLEM TYPES:
Molar conversions
Molar mass of a compound
Isotopic composition
Empirical formula
Molecular formula
Percent composition
Balancing equations
Identifying the type of reaction
PRACTICE PROBLEMS:
1. What is the mass of 3.25 mol Fe2(SO4)3?
2. How many molecules of aspirin, C9H8O4, are there in a 100 mg tablet of aspirin?
3.
How many moles are there in 6.60 g of ammonium sulfate?
4.
Give the molar mass of each compound please,
a. Dinitrogen tetroxide__________________
b. Aluminum carbonate____________________
c. Silver (I) oxide__________________________
d. Lead (IV) sulfate_________________________
5.
Uranium-234 makes up 0.00500 % of uranium atoms and has a mass of 234.041 amu. Uranium235 makes up 0.720 % and has a mass of 235.044 amu. Uranium-238 has a mass of 238.051
amu and makes up 99.275%. What is the average atomic mass of uranium?
6. A compound of silver has the following analytical composition: 63.50% silver, 8.25% nitrogen,
and 28.25% oxygen. Calculate the empirical formula.
7.
An oxide of phosphorus is 56.34% phosphorus, the and the rest is oxygen. Calculate the
empirical formula for this compound.
8. Benzene has an empirical formula of CH and an experimental molar mass of 78 g/mol. What is
its molecular formula?
9.
Determine the molecular formula for a compound with the empirical formula CoC4O4 and a
molar mass of 341.94 g/mol.
10. What is the percentage composition of ammonium sulfate?