Semester One Review Questions
QUESTIONS: Chapters 1-6, 12, 24
1. List steps Scientific Method.
2. Distinguish between mass and weight
3. List Properties SOLID LIQUID GAS
4. What is it called when dry ice becomes a gas? Is this physical or chemical?
5. How does the motion of a solid’s particles differ from that of a gas?
6. How does the motion of a liquid’s particles differ from that of a gas?
7. Identify the following forms of energy as kinetic or potential.
a. Snicker’s candy bar________
b. a galloping horse___________
c. methane gas being combusted___________
d. gasoline in a car tank______________
e. what is the SI unit of energy? ________
8. Estimate the following. Use metric units.
a. mass of your body._______________
b. length of your chemistry book._____________
c. your body temperature_____________
d. volume of a coffee mug.____________
9. How many significant figures are in each number below?
a. .003 ________ b. 1212__________ c. 1200________ d. .0300______
10. Use correct significant figures and units to report the following answers.
a.) 3.24 m x 7.0 m b.) 100.0 g ÷ 23.7 cm3
c.) 0.02 cm x 2.371 cm d.) 710 m ÷ 3.0 s
e.) 1818.2 lb x 3.23 ft f.) 1.030 g ÷ 2.87 mL
g.) 3.24 m + 7.0 m h.) 100.0 g - 23.73 g
i.) 0.02 cm + 2.371 cm j.) 713.1 L - 3.872 L
k.) 1818.2 lb + 3.37 lb l.) 2.030 mL - 1.870 mL
11. Put the following values in scientific notation.
.000098760
1,234,000,000
12.a. Today’s high is predicted to be 18 C. What is this in F?
b. Convert 200.2 degrees Fahrenheit into Kelvin.
13. a. Make the following metric conversion. Study your metric chart. You need to know the numerical value for all the prefixes and be able to convert from one unit to another.
78.53 nm = __________ m
98.3 MHz = __________ Hz
872 hs = __________ s
99,833 μL = __________ mL
9.96 pg = __________ ng
13 b. Use DA to calculate the number of:
cm in 2.3 inches.
sec in 23 days
ml in 1.00 gallon
calories in 5.6 E 23 J
Joules in 569 Calories
14. Difference between homogeneous and heterogeneous mixture give an example of each
15 Classify the following by using the choices a-e
a. colloid b. solution c. pure substance-element
d. heterogeneous mixture e. pure substance-compound
Kool-Aid
Milk and water
Chocolate chip cookie dough
lead pipe
sucrose C12H22O11 (covalent bond)
O3 Ozone (covalent bond)
Cu wire
16.) matching
a. element b. compound c. molecule d. mixture
_____ Simplest form of matter.
_____ Two or more different elements bonded in definite proportions.
_____ Physical blend of two or more substances
_____ a neutral chemically bonded group of atoms that act as a unit.
17) Matching
a. Homogeneous b. heterogeneous c. solution d. colloid e. suspension
____A homogeneous mixture that is made up of a solute and a solvent.
____A heterogeneous mixture that separates over time.
_____Same or uniform throughout
_____not uniform, but different throughout
_____A homogeneous mixture with very tiny particles in it that can refract a beam of light.
18. More Matching
a. solvent b. solute c. alloy d. pure substance
____ A homogeneous mixture of metals
____ the liquid doing the dissolving
____ element, compound, or molecule
____ the particle being dissolved
19 Label each as a chemical or physical change.
a. a marshmallow melts in the fire
b. a marshmallow burns in the fire
c. water boils
d. crushing an Al can
e. fireworks produce beautiful colors
f. sublimation of carbon dioxide
g. building muscle
h. car rusting
i. melting iron
j. digestion
k. sugar dissolving in water
l. tooth decaying
m. grinding coffe
n. ice freezing
o. laundry drying
p. electrolysis of water
19. Draw a Mg atom. Put the correct # of electrons, protons, and neutrons. Put the electrons in their proper energy levels. Label the nucleus.
20. Define isotopes, ions, and give an example of each. Indicate protons, neutrons and electrons for a-d.
#p #n #e
a. Carbon-14
b. 60Co
c. 66 Zn +2
d. 32 P 3-
21. Two isotopes of an element exist. The first has an atomic mass of 33.34 amu and a % abundance of 44%. The second has an atomic mass of 35.00 amu and a % abundance of 56%.
a. What is the average atomic mass of this element?___________
b. What element might this be?_____________
c. What is the atomic # for this element?____________________
22. List the 3 subatomic particles and their properties.
23. What color line spectrum do the following elements produce Na, Sr, K, Cu, Ba?
24. Define electromagnetic radiation and make the electromagnetic spectrum below start with Gamma and continue on to ELF. Label high frequency, high energy, long wavelength short wavelength. Draw a wave, label and define all its properties.
25. For a bromine atom, write the following:
a. electron configuration
b. orbital notation
c. noble gas notation
d. # of unpaired electrons
e. # valence electrons
26. Where is the s,p,d,and f regions of the periodic table?
27. A laser emits light with a frequency of 4.69 E 14 Hz. What is the energy of this radiation?
28. Write a nuclear decay equation for the alpha decay of radium-226.
29.Write a nuclear decay equation for the beta decay of Iodine-131.
30. Calorimeter Problem:
A calorimeter like the one we used in the lab was used to determine the amount of Calories in a marshmallow. Use the data table below to calculate your answers.
Data Table
Find the difference
Mass of marshmallow before burning1.502g after burning .7901g ______
Temperature of Water in ºC before burning 14.0 ºC after burning 31.3ºC ______
Volume of water in Calorimeter 100.0mL before and after
1. Mass of the water in your calorimeter ______________________
2.Temperature change of water_________________
3. Calculate the total calories used to change the temperature of the water in your calorimeter.
________________ Total calories
4. Calculate the calories per gram in the marshmallow.
5. Calculate the Calories per gram in the marshmallow.
6. Determine the percent error if the nutritional label on the bag reads
159Calories/7.2grams.
31. What is a radioactive isotope? Why is it radioactive? What isotopes are radioactive?
32. Explain nuclear fission and nuclear fusion. Give an example of each.
33. A. Read the caliper handed out in class that is labeled A. to find the diameter of a metal sphere. If the sphere weighs 151g determine the density for the sphere.
B. Read the caliper labeled B. to find the diameter of a copper sphere. Determine the mass of the copper sphere if the density of Cu=8.96g/mL.
34. How much heat (in calories) is needed to warm 250 g of water from 22 degrees Celsius to 98 degrees Celsius? The specific heat of water is 1 cal= 1g X 1 degree Celsius
35. How many kJ of heat are needed to raise the temperature of 10.00 kg of liquid water from 24.6 degrees Celsius to 46.2 degrees Celsius?
36. The specific heat of copper metal is 0.385 J=1g x 1 degree Celsius. Is this higher or lower than the specific heat of water? How many calories of heat are needed to raise the temperature of a 1.42 kg block of copper from 25.0 degrees Celsius to 88.5 degrees Celsius?
37. The yellow light given off by a sodium vapor lamp used for public lighting has a wavelength of 589 nm. What is the frequency of this radiation?
38. Calculate the increment of energy that is absorbed or emitted by yellow light. Wavelength= 589 nm
39. Find the density of a piece of metal that measures 5.0cm by 2.0cm by 7.0cm and weighs 489 grams. (use sig. figs)
40. Find the mass for a copper cylider that measures 6cm in diameter and 10cm high. The density of copper is 8.96g/mL (use sig. figs)
Chapter 5/6:
41. Describe a period/series and a family/group
42. Given the elements Rb and Sr, which has the
a. largest radius_________
b. highest ionization energy________
c. highest electron affinity__________
d. highest electronegativity________
43. Given the elements Na and K, which has the
a. largest radius_________
b. highest ionization energy________
c. highest electron affinity__________
d. highest electronegativity________
44. Define the following:
a. radius of an atom
b. ionization energy
c. electron affinity
d. electronegativity
45. Which element is more chemically active?
a. Li or Cs______
b. F or I________
c. Ca or K ______
d. S or Cl_______
46. Label each of the following as a metal, metalloid, or nonmetal.
a. Ca_______ b. Cl_________ c. Kr__________
d. B______ e. As_______ f. Mg__________ g. C__________
h. a substance which is shiny and conducts heat_______
i. a substance which conducts some electricity and is brittle__________
j. a substance which is dull and shatters when hit with a hammer__________
k. a substance that can be drawn into a wire (ductile) ______________
l. a substance that is a good conductor of electricity ______________
m. a substance that loses electrons and becomes a cation __________
47. What are some uses for the following elements (Chapter 6):
hydrogen lithium sodium
potassium beryllium magnesium
calcium strontium barium
chromium iron copper
silver tungsten platinum
boron aluminum gallium
carbon silicon tin
lead nitrogen phosphorus
arsenic oxygen sulfur
fluorine chlorine bromine
iodine helium neon
xenon
48. What metals even in low doses are toxic to humans?
49. List all the family names, first member of each family, group #, # valence electrons, and charge for the main group elements. List the similar chemical and physical properties for that family.
