Download Review-Semester Final (Part I)

Chemistry Review for Semester 1 Exam
1. Label protons, neutrons and electrons in the atoms. Which electrons are the valence electrons?
2. What is the charge of a:
a. proton
b. neutron
c. electron
3. Indicate the number of protons, neutrons and valence electrons for an atom of the following elements:
Li-7
Ca-40
H-1
Ne-20
C-12
N-14
Na-23
Ba-137
Mg-24
O-16
Protons
Neutrons
Electrons
Valence
Electrons
4. Indicate if the following are physical or chemical properties. Label P or C.
_____a. color
______e. physical state
_____b. whether it burns
______f. its reaction with oxygen
_____c. melting point
______g. electrical conductivity
_____d. density
______h. boiling point
5. Label the following as an element (E), compound (C), homogeneous mixture (HM) or heterogeneous mixture (HT).
_____a. CO2
______e. ammonia
_____b. C
______f. O
_____c. salt water
______g. air
_____d. sugar
______h. milk
6. Compare/contrast elements, compounds and mixtures ( smallest unit, how is it broken down?-physical or chemical changes,
examples, pure or nonpure?)
7. Describe the law of conservation of matter (or mass).
8. Find the density for each:
a. 28.0 g and 13.0 mL
b. 35.0 g and 20.0 mL
c. 0.105 Kg and 75.0 mL
9. What is the atomic number for He?
10. What makes up the mass of an atom?
11. What is the atomic mass for He?
12. Calculate the mass of an atom with 10% of Sc-43, 35% of Sc-44, 47% of Sc-45 and the remaining % Sc-46
13. List the 4 signs of a chemical change (i.e. chemical reaction)
14. Give 3 examples of a chemical change and 3 examples of a physical change:
15. Calculate the number of neutrons in the following isotopes:
a. C-14
b. Mg-24
c. Rb-80
16. List 3 elements with a large atomic radius
17. List 3 elements with a small atomic radius
18. Which holds its electrons more tightly- metals or nonmetals? How does this affect the properties of each?
19. Which 2 groups are the most reactive? Why?
20. List two ways that elements in the same group are similar to one another:
21. Why are the noble gases unreactive?
22. Label each as a metal (M), nonmetal (N), transition metal (TM) or semiconductor/metalloid (SC)
a. _________Br
e. _______Na
b._________K
f. _______Ar
c._________N
g. _______Cu
d. ________ C
h. _______Ce
23. Compare/contrast the properties of metals and nonmetals
24. Compare ionic and covalent compounds (use all of the following terms and information: molecular, crystal, ions, molecules,
formula unit, sharing of electrons, gases, liquids, solids, dissolves easily (or no easily) in water, repeating network, high or low
melting/boiling point, conducts (or not) electricity.)
25. The ___________________in an atom are the subatomic particles involved in a chemical reaction. (protons, neutrons, valance
electrons, electrons)
26. What do we call columns of the periodic table? What information is provided by the column #?
27. What do we call rows of the periodic table? What information is provided by the row #?
28. Which compounds are the result of an ionic bond (I) or a covalent bond (C) ?
a. ________KCl
d. ________SO2
g. _______P2O5
b. ________CO2
e. ________C6H12O6
h. _______KBr
c. ________MgCl2
f. ________CaCl2
i. _______SF6
29. What ions (charge/oxidation number) are formed by the following elements?
Na______
Cl______
K______
Al______
N______
H_____
O______
Br______
C______
Mg_____
Ne______
I_______
30. Why does calcium form a +2 ion?
31. Write the lewis dot strucure for :
Mg
Cl
N
O
H
32. Write the lewis dot structure for water, ammonia, methane and O2. Indicate the number of share pairs and lone pairs around each
central atom.
33. a. Write the chemical formulas for:
1. Disulfur hexachloride
b. Give the name for:
1. Au(OH)3
2. Calcium phosphate
2. SO3
3. Ammonium carbonate
3. NH4NO3
4. Chromium (VI) oxide
4. CoCl2
34. What is the shape for:
a. PCl3
e. SCl2
b. CO2
f. N2
c. CH4
g. CHCl3
d. NH3
h. Br2
35. Label the above as polar covalent or nonpolar covalent
36. Put the following intermolecular forces in order of strongest to weakest:
Dipole-dipole forces, Ionic forces, London Dispersion Forces
37. What is a hydrogen bond? Give 2 examples of substances that have hydrogen bonds as an intermolecular force.
38. When intermolecular forces increase, melting points and boiling points ____________________(increase, decrease)
When intermolecular forces increase, vapor pressure ____________________(increases, decreases)
39. Draw an atom of Mg-24, indicating the number of protons, electrons and neutrons.
40. Give the electron configurations for the following elements:
a. Zr __________________________________________ d. Ba_______________________________________________________
b. I
__________________________________________ e. Ag______________________________________________________
c. As __________________________________________ f. Os_______________________________________________________
41. Put Sr, Cr, Fr, Al, F, Cs and P in order of:
a. Largest to smallest atomic radius:____________________________________________
b. Largest to smallest electronegativity:________________________________________
c. Largest to smallest ionization energy:_________________________________________
42. What is the wavelength for electromagnetic radiation with a frequency of 2.04 x 1011 s-1? 3 x 108m/s =c
c= v
43. What is the frequency for electromagnetic radiation with a wavelength of 5.89 x 10-7 m?
3 x 108m/s =c
c= v
44. What is the energy of radiation when the frequency is 8.29 x 10 12 ? 6.626 x 10-34 Js = h
E=hv