Download ATOMIC STRUacad test

Name_______________
Period_______________
Advanced Chemistry-Atomic Structure 1999
I. Multiple Choice-Select the best answer
1. In comparing two compounds of nitrogen and oxygen, it was found that for every 14 grams of
nitrogen in compound A there were 16 grams of oxygen. In compound B, for every 14 grams of
nitrogen, there were 32 grams of oxygen. The ratio of oxygen masses combining with a constant
nitrogen mass in these compounds is therefore 2 to l. Which of the following is illustrated by this
observation?
A. law of conservation of matter
B. law of multiple proportions
C. law of definite proportions
D. Dalton’s hypothesis
2. Which of the following scientists was credited with discovery of the proton?
A. Dalton
B. Thomson C. Millikan D. Newton E. Goldstein
3. Which of the following statements was NOT part of Dalton’s hypothesis on the structure of
matter?
A. All matter is made of atoms
B. Atoms of the same element are identical
C. Atoms are made of protons and electrons
D. Atoms unite in definite ratios to form compounds
4. Which of the following ideas is NOT retained in the current theory of atomic structure?
A. Electrons can absorb or emit energy
B. Atoms have a central, positively charge nucleus
C. Electrons move around the nucleus as planets orbit the sun
D. Most of the volume of an atom is empty space
5. Combining Thomson’s work on the charge-to-mass ratio of an electron with Millikan’s work on
the charge of an electron made it possible to determine the ________
A. Diameter of an electron
B. mass of an electron
C. Pathway of an electron
D. speed of an electron
6. The electric charge and mass number of a electron are, respectively
A. +1 and 1 B. -1 and 1
C. +1 and 0 D. 0 and 1
7. What is the approximate atomic mass of an isotope of sodium that has 11 electrons, 11 protons,
and 13 neutrons?
A. 11 uB. 22 u
C. 13 u
D. 24 uE. 34 u
8. Two isotopes of an element have different ________
A. Atomic numbers B. numbers of electrons
C. mass numbers D. numbers of protons
9. Rutherford’s gold-foil experiment demonstrated that ________
A. electrons have a negative charge
B. most of the atom is empty space
C. X-rays are characteristic of the metal used as the anode
D. energy is given off in little packets
10. Which of the following is an appropriate range for the diameter of an atom?
A. 10-8 cm
B. 10-24 g
C. 1 cm
D. 10 cm
11. Atomic mass is a relative scale based on which of the following nuclides?
A. carbon-12 B. oxygen-16 C. nitrogen-14 D. hydrogen-1
12. What is the mass number of an atom that has 8 protons, 9 neutrons, and 8 electrons?
A. 8 B. 17 C. 16 D. 25
13. The Avogadro constant is ________
A. 2.998 X 108
B. 6.63 X 10-34 C. 6.02 X 1023
D. 1.66 X 10-24
14. Which of the following statements explains why chemists do not count atoms and molecules
directly?
A. Atoms and molecules are extremely small
B. All of the relationships in a chemical reaction can be expressed as mass ratios
C. Matter is neither created nor destroyed in a chemical reaction
D. Reactions occur one atom at a time
15. The basic principles of atomic theory that are still recognized today were first conceived by
A. Avogadro B. Bohr
C. Dalton
D. Rutherford
16. Dalton’s atomic theory helped to explain the law of conservation of mass because it stated that
atoms:
A. could not combine
C. could not be created or destroyed
B. all have the same mass
D. are invisible
17. The law of multiple proportions was proposed by
A. Avogadro B. Rutherford C. Thomson
D. Dalton
18. An example of the law of multiple proportions is the existence of
A. H2O and H2O2
B. O2 and O3 C. FeCl3 and Fe2(SO4)3
D. FeCl2 and Fe(NO3)2
19. In Rutherford’s experiment, a very few of the positively-charged particles were
A. slightly deflected as they passed through the metal
B. greatly deflected back from the metal
C. passed straight through the metal
D. combined with the metal
20. The artificial hydrogen isotope with the highest mass is named
A. tritium
B. deuterium C. hydrogen D. protium
21. Atoms of the same element can differ in
A. chemical properties
B. atomic number
electrons and protons
22. Most of the mass of an atom is concentrated in the
A. electron cloud
B. nucleus
C. neutron
C. mass number D. number of
D. proton
23. Carbon-14 has 8 neutrons. What is the atomic number of carbon-14?
A. 14 B. 8 C. 12 D. 6
24. Oxygen-18 has an atomic number of 8. How many neutrons does this isotope have?
A. 8 B. 24 C. 10 D. 18
25. Neon has an atomic number of 10. Calcium has an atomic number of 20. Compared to a mole of
neon, a mole of calcium contains
A. twice as many atoms
B. half as many atoms
C. an equal number of atoms
D. 20 times as many atoms
II. Matching
26. Chadwick
27. Isotopes
28. Curie
29. Thomson
30. Rutherford
A. Radioactivity
B. discovered neutron
C. Gold Foil Experiment
D. discovered the electron
E. C-12, C-14
31. Proton
32. Law of Multiple Proportions
33. Bohr
34. electron
35. Neutron
A. –1,1
B. CO,CO2
C. +1, 1
D. Planetary model
0,1
Periodic Table Questions:
_____ 36. The element located at position period 3 and column IVA is
a. Pb
b. Cu
c. Si
d. Ga
_____37. . The element located at position period 5 and column VA is
a. Bi
b. Sb
c. Si
d. Sn
_____38. The element located at position period 2 and column IIIA is
a. Ca. b. B
c. Ca. d. Zn
_____39. What element and group is phosphorus in?
a. Period 1,group IVA b. Period 2, group IIB
c.Period 2, group IA d. Period 3, group VA
_____40. What is another name for group IA on the periodic chart?
a. Alkali metals b. halogens c. noble gases d. carbon family
Conversions:
Grams to molesor Convert Moles to grams
_____41. How many moles are in 81 grams of beryllium?
a.12
b. 16 c. 9 d. 1.9
_____42.How many moles are in 48 grams of oxygen?
a.4 b.9
c.3
d.13
_____43. Change 6 moles of Potassium to grams
a. 234 grams of Potassium b. 342 grams of potassium
c. 123 grams of Potassium d. 407 grams of Potassium
_____44. Convert 4 moles of Flourine to grams.
a. 76 grams b. 23 grams c. 4.75 D. none of the above
_____45.Convert 3 moles of Sodium to grams.
a. 40grams
b. 69 grams c.56grams
36. How many moles are in 42.6 g of Mg?
A. 102.2 moles
B. 85.2 moles
C. 94.7 moles
D. 1.75 moles
d. 72 grams
Convert moles to # of atoms or # atoms to moles
_____46.How many atoms are in 3 moles of sodium?
a. 6.02x10 23 b.14.09x10 23 c.18.06x1023 d. 12.04x1023
_____47. How many moles are in 1.2 X 1024 atoms of Zn?
A. 1.00 moles
B. 2.00 moles
C.
3.00 moles
_____48. How many atoms are in 4.2 moles of Ne?
A. 6.9 x 1023
B. 6.9 x 1024
D. 4.00 moles
C. . 2.5 x 1023
D. 2.5 x 1024
_____49. How many atoms are in 4.2 moles of Ne?
A. 6.9 x 1023
B. 6.9 x 1024
23
C. . 2.5 x 10
D. 2.5 x 1024
_____50. How many atoms are in 4.2 moles of Ne?
A. 6.9 x 1023
B. 6.9 x 1024
C. . 2.5 x 1023
D. 2.5 x 1024
III. Problems-SHOW WORK AND FACTOR LABEL or no credit
1. How many grams of antimony are in 3.42 moles of antimony
2. How many atoms are in 6.12 grams of potassium?
3. How many grams of tin are in 3.1 x 1024 atoms?
IV. Fill in the blank
Ion or Isotope
Element
Symbol
Atomic
#
Mass #
#P
#N
#e-
_______
______
F-
______
19
___
____
____
_______
2H
______
2
____
____
0
_____
_____
____
32
___
_____
_______
____
____
10
_____
Nickel
_______
28
-3
15
Charge
_____6. Which element is located in period 6 , group IIIA?
a. Ca b. K c.Ti d. Mg
_____7. Go to period 4 group VIA. What is the element’s symbol?
a. Se b. Kr c. As d. Ge
____8. What element is located in period 3, group IIA?
a. Mg b. Na c. Mn d. Fe
_____9. Which element is located in period 5, group IIB?
a. w b.Ag c.Mo d.Cd
_____10. Which element is located in period 2, group VIA?
a. S b. Se c. O
d. Te
_____16. Convert 2 moles of Sodium to grams.
a. 46g
b.23g
c.36g d.48g.