Download Chemical reaction chapter test study guide

SCIENCE 8CP
Name: ___________________ Period: ____
Chemical Reactions Test Review Sheet KEY
1. Calculate the number of atoms of each element shown in each of the following:
a. CaSO4 ___6_____
b. 2 NaCl
__4______
c. Fe(NO3)2 __9______
d. Al2(CO3)3 ____14____
2. Balance each of the following equations:
a. ____ Na2CO3 + _2___ HCl → _2___ NaCl
+ ____
H2O + ___ CO2
b. _2__ HCl + ____ Cr → ____ CrCl2 + ____ H2
c. ____ F2 + __2__ KCl → __2__ KF + ____ Cl2
3. What happens in an exothermic reaction? ___Energy is released/produced from reaction______________
Would an exothermic reaction get HOT or COLD? (Circle one)
4. What happens in an endothermic reaction? ___Energy is absorbed/needed for reaction______________
Would an endothermic reaction get HOT or COLD? (Circle one)
5. Name four ways you can increase the rate of a chemical reactions.
a. Increase temperature
c. Increase surface area
b. Increase concentration
d. Add a catalyst
6. Name four clues or indicators that a chemical reaction occurred.
a. Explosion
c. Gas produced
b. Temperature change
d. Precipitate formed
7. List the five types of chemical reaction:
a. Synthesis
b. Double Replacement
c. Decomposition
d. Single Replacement
e.
Combustion
8. Identify the types of reactions shown in each of the following equations:
a. 2 H2 + O2 
2 H2O Synthesis
b. 2 Al + NiBr2  AlBr3 + Ni
Single Rep.
c. AgNO3 + KCl  AgCl + KNO3 Double Rep,
d. 2 H2O2  H2O + O2
Decomposition
9. Why can’t you change the subscripts in a chemical formula? Changing the subscripts would change
the identity of the substance.
10. Label the reactants, products, coefficients and subscripts in the following reaction:
REACTANTS
2 K + MgBr2 
Coefficients
PRODUCTS
2 KBr + Mg
Subscripts
11. What does the Law of Conservation of Mass state?
Mass cannot be created or destroyed. The number of atoms of reactants must equal that of products
12. Balance the following reaction with POLYATOMIC IONS: ___ FeCl3 + _3__ NaOH  ___ Fe(OH)3 + _3_NaCl
3 1
OH
3
3 1
Na
1
3
1
Fe
1
3
Cl
1 3
MAKING THINGS STRONGER VIDEO QUESTIONS
1. List two elements found in steel. ________carbon and iron____________________________
2. What is “tensile strength?”
________maximum stress a material can take before it breaks_________________________
3. What is “compressive strength?”
_________ability to withstand pressure (chalk, ceramics)_______________________________
4. What are nanotubes made of? ______ carbon ____________________
5. True or False: Spider silk has more tensile strength than steel. TRUE
CARBON BASED MOLECULES (Macromolecules)
1. What is organic chemistry? ______study of living (or once living) organisms_____________________
2. What properties of carbon makes it the building block of life?
_____ability to bond with many elements, backbone of long, complex chains, a lot things made of it___
3. What are three examples of pure carbon? _____graphite, diamond, wood___________________
4. How many valence electrons does carbon have and what would the Lewis Dot Diagram look like?
4 valence electrons
5. Identify the monomer for each organic molecule. (ex. proteins – amino acids)
Proteins – amino acids; Carbs– monosaccharides; Nucleic acids – nucleotides; Lipids – fatty acid
6. What foods are examples of carbohydrates, lipids and proteins?
Carbs: Pasta, breads, starches; Proteins: meats, eggs, cheese; Lipids: butter, oil
7. What is a monomer? __molecule that bonds together to form a more complex polymer____
8. What is a polymer? _____macromolecules, larger more complex molecules formed from
monomers_____
ACIDS AND BASES
1. Know the chemical formulas for the five common acids (ex. Nitric, phosphoric, etc.)
Acetic acid CH3COOH, Hydrochloric acid HCl, Nitric acid HNO3, Sulfuric acid H2SO4
Phosphoric acid H3PO4
2. What is the pH range for acids? What about bases? Acids pH = 1-6, Bases pH = 8-14
3. What are three characteristics of acids? What are three characteristics of bases?
Acids are sour, corrosive and typically plot in the red/orange range
Bases are chalky, bitter and typically plot in the blue/purple range
4. What is the pH for a substance that is neutral? What is an example of a neutral substance?
____Neutral pH = 7; water, blood_______________________________
5. Know the definition of Bronsted-Lowry acids. _____Acid- proton donor, Base= proton acceptor______
6. Identify the acid, the base, the conjugate acid and the conjugate base in the reaction:
NH3 (g) + HOH (l) ⇄ NH4+(aq) + OH-(aq)
Base
Acid
C.A.
C.B.
7. Identify the acid, the base, the conjugate acid and the conjugate base in the reaction:
HCO3 -(aq) + HOH (l)
Acid
Base
⇄
CO3 2-(aq) +
C.B.
H3O+ (aq)
C.A.