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Chemistry - Mid Term Exam Review Sheet #
The midterm exam covers chapters I - 4 & 9 - I I. You should read through each chapter, look over old tests you still
have. answer the l~llowing questions and do the calculations in order prepare yonrself Ibr the mid-term.
I. Define tbc l~llowing terms and describe where each is located.
proton -
neutron -
electron --
- Complete the following table:
Element name Atomic #^ Mass^ # of protons^ # of Neutrons^
of Electrons Symbol
Hydrogen
Carbon
Sodium
Calcium
Fe
- Define the following and give an example of each using chemical symbols.
atomic number /
atomic mass /
isotope /
- Which of the following are isotopes of the same element?
199y 2%y 1910 Y
5. Describe Rutherford’s experiment:
- Explain all the major parts of Dalton’s Atomic Theory.
b.
d.
- Balance the following chemical equations:
CO + Fe203 --) Fe (^) + CO
ZII(OH)2 + H3PO4 "-) __ ZI13(PO4)2 + H
- Define Ionic and Molecular componnds, and tell how each is formed.
- Name the following compounds and state if it is ionic or molecular in nature:
a. AI(OH)
b. N2Os
c. MgI
d. (^) C
Chemistry - Mid Term Exam Review Sheet #
- Write a chemic al formula for each nanle given and tell whether it is an ionic (i) or molecular (m) compound:
a. Aimnonium Phosphate
b. Magnesinm Nitride
c. Oxygen Difluoride
d. Carbon Dioxide
e. Sulfur Dioxide
1 I. Name and describe the 6 types of chemical reactions. Give all example of each.
b.
d.
f.
- Define and give all example of each:
Element (^) /
Mixtnre (^) /
Compound (^) /
homogeneous substance /
heterogeneous substance /
physical property /
chemical property /
physical chauge /
chemical change /
q ualitative measurements /
qnantitative measurement (^) /
- Which of the followiug is a homogeneous mixtnre?
a. oil ill water b. soot ill water (^) c. alcohol in water
- Which of the followiug could be considered a physical change?
a. cooking a pancake b. burning a tree c. melthag an ice cube
- Which of the following is considered a heterogeneous mixture?
a. salt and sugar b. flour and baking powder (^) c. salt aud pepper
- Classify each as a physical or chemical change.
__ a. instant coffee is combined with hot water to prodnce a brown liquid
__ b. from exposure to air and moisture, iron turns reddish and cannot conduct electricity
c. iron is heated, turns red and then melts
__ d. sugar is heated to produce steam and a black solid
Chemistry - Mid-Term Exam
Study Guide: 2
Name
Per.
I I. What is the total positive charge on the Aluminum ion in the following compounds?
a. A1(CIO4)3 ____ b. AI2(SO_~)3 __ c. AIPO,~
- For each compound in question # 25 give the following inlbrmation:
Al(ClOa)3 AI_~(SO_Oa^
AIpOa
of moles of atoms for
each element
the total number of atoms in
the entire compound
gram molecular mass of
compound
- What is Avogadro’s nmnber? 6.02 x 10
2~
- Define the following:
Molecule
Atom
Ion
Cation
Anion
- From what type of elements are cations and ~nions formed and explain how each is formed.
Cations: metal - loss of electron(s) (-)
Anions: nomnetal - gain electron(s)
- Calculate the % composition by mass of the componnds formed from these reactions.
a. 8.2 g of Mg combine with 5.4 gofoxygen Mg- 60.3% - O = 39.7%
b. 29gofAgcombinewith4,3gofsulfnr Ag=87.1%^ -^ S-12.9%
- Calculate the % composition by mass
PropaneC~Hs C=81.2% H= 18.9%
W~.ter H I1.1% O-88.9%
- Element X has two isotopes. The first isotope has a mass of 10,012 amu wiih a relative abundance of 19,91%. The secgnd
has a mass of 11.009 and has a relative abundance of 80.09%. Calculate the -atomic mass of this dement, and name it.
!9. The four isotopes of lead are given below, each with its percent by mass abundance and the composition of its nucleus.
Using this data, calculate the atomic mass of lead.
Pb Pb^
Pb Pb
p+ =82 p+ =82^ p+-82^ p+ 82
n
= n=124 n 125^ n-
1.37% 26.26%^ 20.82%^ 51.55%
Mass>
Hint: for # I 7, and 18 use the formula: % mass (of each element)^
= grains of element
x 100%
grams of compound
Chemistry - Mid-Term Exam
Study Guide: 3
- A copper penny bas a mass of 3.1 g and a volunae of0.35cm
What is tbe density of copper?
2.A liquid has a density of 4.8 g/ml. What is the mass ofa 2 liter sample?
- What is the volume of a substance that has a mass ors0 g and a density of 10 g/cm3?
- Indicate the meaning (as a power of 10) for each of the following metric prefix:
a. kilo b. centi
d. deci e. nano
- Calculate the following quantities:
a. 1,100cm
= (^) m b. lm -
d. 2.5km - m.^
e. 4.05kg:
g. Inm = m^ I1.3.0^ g
- Indicate tbe nnmber of significant figures in each of the following:
a. 12600 b. 0.09 c. 200 I
- Define:
accuracy
precision
c. milli
f. Micro
111111 C, i0 Ill :
g (^) f. 0.5g
ng
d. 0,00500100 e. 1000
cm
mg
- The accepted value or true value for the density of lead (Pb) is 11.35 g/ml. Your experimental value or observed
value found during a class lab is 9.65 g/mL
What is the error of your measurement?
What is the percent error of your measurement?
- Define:
Meter
Liter
Volume
Mass
Grain
Temperature
- Name the two temperatnre scales nsed in science? Give the freezing pt., and boiling pt. of water foreach of theln.
I 1. Which type of particle (atom, ion, or molecule) goes with each oftbe following substances?
a. Na b. Ca
c. N
d. CI~ e. H20 f. CO
- Define:
empirical formula
molecular formula
- Which of the following are empirical formulas and which are molecular formulas?
a. CH4N b. NaO^ c. C~H3Os
