Download 1st Term Review

Chemistry 1 Midterm Review #1
1. Name the scientist(s) responsible for each of the following. You may use a scientist more than once.
a) The plum pudding model of the atom
b) Modern atomic theory
c) Modern periodic law
d) Discovery of the nucleus
e) Discovery of the neutron
f) Gold foil experiment
g) Father of the modern periodic table
h) Discovery of the electron
i) Atomic model of hydrogen
2. How do isotopes differ from one another?
3. List the periodic trend for the following (across the chart from left to right and down a column)
a) Ionization energy
b) Electronegativity
c) Atomic mass
d) Atomic radius
4. List the elements which are metalloids.
5. List four physical properties of metals.
6. List the diatomic elements.
7. Consider the element located in period 5, group 11. How many moles are equivalent to 455 grams of this
element?
8) 2.375 moles of Cu = _________ g Cu
9. According to the Bohr model, why does a hydrogen atom produce a line spectrum and not a continuous
spectrum?
10. How many mL are in 0.45 liters? (1000 mL = 1 liter)
11. What element has the following electron configuration? 1s22s22p63s23p64s23d104p65s24d5
12. Dalton believed that all atoms of the same element are exactly alike. What discovery has since proved that
untrue?
13. What is the mass of grams of 0.500 moles of Au?
14. Based on the gold foil experiment, what did Rutherford conclude about the atom?
15. An atom of chromium-60 contains how many protons, neutron and electrons?
16. What is the difference between a compound and an element?
17. What is the electron configuration of a neutral calcium atom?
18. Atomic mass is measured in atomic mass units (amu) that are based on one atom of which isotope?
19. Thomson’s cathode ray tube experiment led to the discovery of what?
20. According to quantum theory, when will an atom radiate a photon of light?
21. Balance the following nuclear reaction equations
a) potassium-40 undergoes beta decay (electron)
b) uranium-238 undergoes alpha decay
22.
Symbol
201
80
Hg
60
28
Ni
Protons
4
47
Neutrons
5
61
Electrons
Charge
0
0
23. Write the electron configuration notation and Lewis dot notation for Chromium (Cr).
24. Write the noble gas notation (shorthand notation) and Lewis dot notation for Antimony (Sb).
25. Draw the Lewis structure and state the molecular geometry and bond angle for each of the following.
a) H2O
b) CO2
c) SiF4
26. Write the formula for each of the following compounds.
a) Sulfur hexafluoride
b) Lithium nitride
d) Tin (II) chloride
e) Ammonium acetate
g) Potassium bromate
h) Sulfurous acid
j) Hydrosulfuric acid
k) Chloric acid
27. Name each of the following compounds.
a) CuSO4
b) AlF3
c) HI
g) HNO2
h) NaHSO4
c) Chromium (III) carbonate
f) Mercury (I) chloride
i) Dinitrogen pentoxide
l) Magnesium hypochlorite
d) NO
e) H2Se
f) HNO3
28. Tritium (H-3) is a radioactive isotope of hydrogen with a half-life of 12.3 years. How long would it take for
a 40.0 g sample to decay down to 1.25 g?
29. Fe-61 has a half-life of 6.00 min. Of a 100.0 mg sample, how much will remain after 18.0 min?
30. How many moles are in each of the following amounts?
a) 64.1 g of aluminum (Al)
b) 8.08 x 1022 atoms of krypton (Kr)
31. Calculate the mass of the following quantities.
a) 8.022 x 1023 atoms of Ta
b) 64 L of Cl2
c) 45 L of ammonia (NH3)
c) 17 moles of NH4NO3
32. Calculate the number of representative particles in each amount.
a) 45 g of lithium chloride (LiCl)
b) 1.25 moles of carbon tetrahydride (CH4)
c) 24 L of xenon (Xe)
33. A compound is found to have 46.67% nitrogen, 6.70% hydrogen, 19.98% carbon and 26.65% oxygen. What
is its empirical formula?
34. A compound is known to have an empirical formula of CH and a molar mass of 78.11 g/mol. What is its
molecular formula?
35. Determine the percent aluminum in Al2(Cr2O4)3.
36. Determine the percent water in CaSO4 · 2H2O.
37. A compound is found to have (by mass) 48.38% carbon, 8.12% hydrogen and the rest oxygen. What is its
empirical formula?