Semester 1 Study Guide – Pre AP
Unit 1
3. What is the difference between quantitative and qualitative data? (Know definition of both)
4. What is the difference between accuracy and precision? (Know definition of both)
5. What type of relationship do two variables have when if one goes up, the other also goes up?
6. What type of relationship do two variables have when if one goes up, the other goes down?
8. Convert the following:
.44526 nL to pL _______________________
57,083 mg to kg ________________________________
37.67 µg to kg ________________________ .0093 m to nm _________________________________
11. The accepted value of the density of water is 1.0 g/cm3. If you calculate the density of water to be 1.7 g/cm3, what
is your percent error?
12. Calculate the density of mercury if the mass of a sample is 53 g and occupies a volume of 4.9 mL.
13. What is density?
15. Convert: 53OF to OC
16. Convert 25OF to K
17. Convert 370 K to OF
19. Find the volume of a sample of nickel that has a density of 10.92 g/cm3 and weighs 550 mg.
20. Convert:
100 cm to inches ______________________
27 miles to kilometers ____________________
21. Know what the four descriptions of precision and accuracy are and be able to identify them (accurate but not
precise, both accurate and precise……)
23. Put in scientific notation:
.000000456
____________________
132500000000000
5300
____________________
.0000000000000000084 __________________
Unit 2
1. What is matter?
3. What two things must an object have in order to be considered matter?
9. What is Melting? Freezing? Evaporation? Condensation?
10.How is a chemical change different from a physical change?
11. Label the following as either a physical or chemical change:
A. Iron rusting B. Wood rotting -
___________________
C. Chlorine gas condensing into a liquid D. Melting cheese E. Burning paper F. Freezing Water G. Mixing sugar in water 14. What is the difference between a homogeneous and heterogeneous mixture? Give an example of each.
15. What is energy?
16. If you raise the temperature of something, what will its particles do?
17. What is an endothermic reaction? Give an example.
18. What is an exothermic reaction Give an example.
20. What is the SI Unit for energy?
22. What is the specific heat of water?
23. What is specific heat?
24. Find the velocity of a train that has a mass of 500,000 g and has a KE of 2,000,000 J.
25. Find the thermal energy of a lake that has a mass of 1,000,000 g and decreases in temperature from 40 OC to 30 OC.
26. Why does water have such a high specific heat?
Unit 3
1) What is an atom?
2) Who was the originator of the atomic theory?
3) This is a dense region of the atom that has a positive charge. Why does this region have a positive charge?
4) Explain the relationship between the mass of a neutron and the mass of a proton.
5) Atoms of elements have a mass unit called the amu (atomic mass unit). What atomic particles affect an atoms’
amu?
6) This is the region where electrons reside.
7) What is the charge of a proton? Neutron? Electron?
8) Protons and electrons of an atom are equal to what?
9) How do you calculate the number of neutrons in an atom?
10) This is an atom of an element that has a different mass. Why does this atom have a different mass?
11) Find the number of P, N, and E in Carbon – 12 and Carbon – 13
12) Who created the periodic table
13) What is a mass number?
14) Approximately how many elements on the periodic table are naturally occurring?
15) How many groups on the periodic table?
16) What does the group number tell us about an atom?
17) What does the period number tell us about an atom?
18) Tell me names for the following groups:
Group 1:
Group 2:
Groups 3-12:
Group 13:
Group 14:
Group 15:
Group 16:
Group 17:
Group 18:
19) Give me the names of the following periods:
Period 6:
Period 7:
20) What is a valence electron?
21) How many valence electrons on the:
1st energy level:
2nd energy level:
3rd energy level:
23) Show me the LDS of :
Li
Br
Se
Al
Si
Ar
25) What is a diatomic element?
26) Name the 7 diatomic elements:
27) Find the number of neutrons in barium
29) What is a metalloid? What is a metal? What is a nonmetal?
30) Find the average atomic mass of lithium if 7.42% exists as Lithium – 6 and 92.58% exists as Lithium – 7
32) Find P, N, and E of:
28
13 Al
34) Draw an energy level (Bohr) diagram for the following elements:
H
B
Al
35) What determines the reactivity of an atom?
9. How many electrons does the F orbital hold? D orbital? P orbital? S orbital?
12. Write the noble gas notation of gallium, lead, and californium
13. Write the orbital notation of Rhenium, Strontium, and Ytterbium
14. Write the electron configuration diagram for Os, Pt, N-3, Ar, and Na+1
16. Find what is wrong the following orbital notations and explain (use a rule or principle if that applies) :
b) 1s22s22p63s23p64s23d104p65s24d105p66s25d10
c) 1s22s22p63s23p64s24d104p65s24d105p66s2
8. Po – 209 has a half life of 103 years. If you have a 500 g sample, determine how many grams would be left after 4
half lives. How long would it take for that 500 g sample to be reduced to 3.90625 g.
12. If you have 5 grams of Carbon – 14 in a bone sample with a half life of 5,730 years, how old would the bone be if
you knew that there were originally 160 g of Carbon – 14 in the bone sample?
16. Write the following isotopes using nuclear notation:
Uranium-235 ________
Lead- 207__________ Cobalt-60 _________ Cesium-137 ___________
Potassium-37 ________ Plutonium-239 _________ Strontium-90 __________
17. H3 (tritium) is an artificially produced radioisotope used in some nuclear reactions. How much
of a 1.000 kg sample remains after 85.82 years (half life = 12.26 yrs)?
Unit 4
____________________1. Write the chemical formula for aluminum sulfate.
____________________2. Calculate the molar mass of aluminum sulfate.
____________________3. Determine the percent by mass of aluminum in aluminum sulfate.
____________________4. Determine the percent by mass of sulfur in aluminum sulfate.
____________________5. Determine the percent by mass of oxygen in aluminum sulfate.
___________________6. How many moles are in 15.8 g of aluminum sulfate?
___________________7. How many grams are equal to 0.215 mole of aluminum sulfate?
___________________8. How many grams are equal to 2.05 x 10 25 molecules of aluminum sulfate?
Unit 5
2. Determine the following for the comparison between Li and F and explain why:
Largest Atomic Radius –
Largest Ionic Radius –
Highest Electronegativity –
Highest Ionization Energy 3. What are Coulomb’s Forces? Compare the atomic radii of Bromine and Selenium and explain how Coulomb’s forces
play a part.
4. What is a cation? What is an anion? How do these two affect ionic radius?
5. What is electronegativity? What is ionization energy? What is atomic radii? What is ionic radius?
6. Compare the atomic radii, electronegativity, ionic radius, and ionization energy of chlorine and sodium. Tell which
element is larger in each of those 4 categories and explain why for each section.
7. You have two elements. One of them has 17 protons and 17 electrons. One has 16 protons and 17 electrons. Explain
which element is smaller and tell why.
8. Why does the trend for ionization energy decrease as you go down the periodic table?
9. What is an oxidation number and how does it play into electronegativity and the desire to acquire electrons.
12. What is an ionic compound? What is a covalent compound? Provide an example of each and be able to explain the
difference between them and explain what happens in each compound. Also be able to identify whether a compound
is covalent or ionic.