This document defines key chemistry terms and concepts related to aqueous solutions, electrolytes, acids and bases, precipitation reactions, and solubility. It asks the student to identify strong acids and bases, ions present when various substances dissolve in water, solubility of compounds, precipitation reactions, and classification of solutions as nonelectrolytes, weak electrolytes, or strong electrolytes. The document provides a review of general chemistry topics through multiple choice and short answer questions.
This is a small presentation designed around Lewis Numbers. The content would be appropriate for a grade 10 Physical Science learner, in a CAPS curriculum school.
This is a small presentation designed around Lewis Numbers. The content would be appropriate for a grade 10 Physical Science learner, in a CAPS curriculum school.
Chem 101 Spring 2017 Name _______________________________.docxchristinemaritza
Chem 101 / Spring 2017 Name: ______________________________________
Exam 2 // 198pts Lectures H through L (199)
1. Multiple Choice: Choose the best answer and put the number in the blank provided. (45pts)
A. _______ Compounds that have only non-metal element and only covalent bonds are
1. Didactic 2. Nobel Compounds 3. Ionic 4. Molecular
B._______ The Atomic Mass on the periodic table is:
1. The mass of the protons in an atom 2. The mass of a mole of atoms of a given element
3. The mass of an atom. 4. The Mass of a mole of protons
C._______ What is the major attractive force in a compound like NaCl?
1. Dipole-dipole, 2. London dispersion, 3. Ionic, 4. Hydrogen bonding
D. _______ Which of the following represents an Empirical Formula
1. N2O6 2. C6H12O6 3. C2H4 4. SO3
E. _______Atoms of the Non-metal elements generally form ions by
1. Losing electrons, forming positive ions 2. Losing electrons, forming negative ions
3. Gaining electrons, forming positive ions 4. Gaining electrons, forming negative ions
F. _______ The Atomic Mass Unit (AMU) is the mass of
1. A Mole of Carbon 2. A Hydrogen Atom 3. A Carbon Atom 4. An Electron
G. _______ A Polar Covalent bond has a
1. Random Charge 2. Positive Charge 3. Negative Charge 4. Dipole
H._______ Reaction ratios in gas phase reactions can be measured by
1. Temperature 2. Color 3. Volume 4. Time
I. ______ The formula showing the total number of each elements in a chemical formula is the
1. Molecular Formula 2. Atomic Formula 3. Thermodynamic Formula 4. Empirical Formula
J. ______ Which of the following would have the highest melting temperature?
1. H2O, 2. CO2 3. SO2 4. MgF2 5. NH3
K. ______ Carbon is very good at forming covalent bonds because
1. It is the best at forming Ionic Compounds 2. Its electronegativity is mid-range
3. Its electronegativity is very large 4. Its electronegativity is very small
L. ______ Ionic Compounds
1. Have poor solubility in water 2. Usually have low melting points
3. Conduct electricity when in solution 4. Readily form molecules
M. _____ The weakest of the intermolecular forces are:
1. Ionic 2. Covalent 3. Electron sea model 4. Dipole / Dipole 5. London
N. _____ Which statement is true about Hydrogen Bonds?
1. They are stronger than covalent bonds 2. They are the weakest of all interactions
3. They are stronger than ionic bonds 4. They are weaker then covalent bonds
O. _____ The physical properties of metals result from the inter-particle forces called:
1. Ionic 2. London 3. Electron sea model 4. Covalent 5. Dipole / Dipole
P. ______ Ionic compounds dissolve in water because the ions in the compound
1. Attract 2. Repel 3. Negate 4. Dissociate
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Chem 101 / Spring 2017 Name: ______________________________________
Exam 2 // 198pts Lectures H through L (199)
Q. ______ In the kinetic molecular theory gas particles are
1. Far apart 2 ...
I use this lab sequence over a couple of lessons to get to grips with some basics of different types of reactions, balancing, writing formulas and problem-solving.
1. GENERAL CHEMISTRY-I (1411)
S.I. # 12
1. Define the following:
a. Aqueous Solution:
b. Solvent:
c. Solute:
2. Define the following:
a. Electrolyte:
b. Nonelectrolyte:
c. Strong Electrolytes:
d. Weak Electrolytes:
e. Solvation:
3. What is a precipitation reaction?
4. Define the following:
a. Molecular Equation:
b. Complete ionic equation:
c. Spectator ions:
d. Net Ionic equation:
5. Define the following:
a. Acids:
b. Bases:
6. List the following: Strong Acids Strong Bases
1. ___________ ___________
2. ___________ ___________
3. ___________ ___________
4. ___________ ___________
5. ___________ ___________
6. ___________ ___________
7. ___________ __________and __________
2. 7. Specify what ions are present upon dissolving each of the following substances in
water:
a. MgI2
b. Al(NO3)3
c. HClO4
d. KC2H3O2
8. Predict the solubility of the following compounds in water:
a. Ni(OH)2 ________
b. PbBr2 ________
c. Ba(NO3)2 ________
d. AlPO4 ________
e. AgC2H3O2 ________
9. Identify the precipitates that form (if any) when the following solutions are mixed
and write a balanced equation for the reaction.
a. Ni(NO3)2 with NaOH
b. NaOH with K2SO4
c. Na2S with Cu(C2H3O2)2
10. Write balanced net ionic equations for the reactions that occur in each of the
following cases and identify the spectator ions in each case.
a. Cr2(SO4) (aq) + (NH4)2CO3 (aq)
b. Ba(NO3)2 (aq) + K2SO4 (aq)
c. Fe(NO3)2 (aq) + KOH (aq)
11. Classify each of the following aqueous solutions as a nonelectrolyte, weak
electrolyte, or strong electrolyte:
a. HClO4 ________ b. HNO3 ________ c. NH4Cl ________
d. CH3OCH3 ________ e. CoSO4 ________ f. C12H22O11 ________
g. H2SO3 ________ h. C2H5OH ________i. NH3 ________
j. KClO3 ________ l. Cu(NO3)2 ________