Download Unit 2 Practice Exam exam_2p_08_matter

Exam 2 Practice - Atoms, Radioactivity, Electrons, Periodic Table
Labs - Distillation, Shielding Radioactivity, Alchemist’s Dream, Flame Tests
Dalton’s atomic theory – basis, main points, explanations, updates
Experimental discovery of electron, Discovery of Nucleus,
Bohr Model & Absorption & Emission of Light & Spectral lines
Drawing Bohr models vs Quantum Mechanical Models
Radioactivity, 1/2 Lives, Nuclear Equations & Applications of Nuclear Chemistry
Charge Cloud Model, Orbitals & Electron Configurations
Periodic Patterns of electrons and their properties of elemental groups.
Graphing - see your lab report grading rubric for graphing guidelines
1. Complete the table below
Element
Atomic #
Q
12
R
S
Atomic Mass
Protons
46
22
34
Neutrons
13
Electrons
14
Charge
+2
-1
37
2.
Write the isotope symbol for R.
3.
What change would be required to change element Q to the same as element R?
4. Which of the following corresponds to observations made by Rutherford’s team?
a. atoms are mostly empty space.
b. the positive charge of an atom is concentrated in a nucleus.
c. alpha particles that hit the zinc sulfide film produced sparks
d. if the plum pudding model is true, then alpha particles will pass straight through or be deflected slightly.
5. Which of the following scientific laws was Dalton able to explain as due to atoms simply rearranging in a chemical
reaction?
a. Law of Conservation of Energy
b. Law of Definite Composition
c. Law of Conservation of Mass
d. Law of Multiple Proportions
6. Which of the following was NOT a key point of Dalton’s atomic theory?
a. atoms are indivisible and indestructible.
b. atoms are mostly empty space.
c. atoms of an element are identical in mass.
d. atoms combine in simple whole number ratios to form compounds.
7. Which of the following is NOT an update to Dalton’s atomic theory?
a. Atoms are divisible and composed of smaller particles.
b. Atoms can be converted into other types in a nuclear reaction.
c. Atoms of an element are not identical and can differ in mass.
d. Atoms of different elements are different in mass.
8. How did Thomson know that electrons are found in all types of matter?
a. Cathode rays originated at the cathode.
b. Cathode rays are attracted toward a positively charged electrode.
c. Cathode rays are not light.
d. Thomson observed the same behavior of cathode-ray particles using a variety
of gases in the Crookes tubes and a variety of materials for electrodes.
9. Who discovered the electron?
a. J.J. Thomson
b. Ernest Rutherford
c. Neils Bohr
d. Dmitri Mendeleev
10. What evidence indicated that each atom has a nucleus?
a. When alpha particles are shot at gold foil some alpha particles are deflected
slightly or at large angles.
b. Each time an alpha particle hit this zinc sulfide coating, a flash of light was
produced at the point of contact.
c. Positively charged alpha particles were deflected rather than attracted by the
gold nuclei.
d. Nearly all the alpha particles passed straight through as though there were no
foil there.
11. How do atoms emit specific colors of light?
a. The farther from the nucleus the more energy an electron has.
b. Electrons tend to occupy the lowest possible energy levels.
c. When excited electrons drop back down to lower energy levels it releases light
of corresponding energy.
d. When an electron absorbs a specific amount of energy it will be boosted to a
higher energy level.
12. What did the discoverer of the nucleus think that an atom looked like?
a. Positive and negative charges are distributed evenly throughout the mass of an
atom like plums in plum pudding.
b. Electrons orbit the nucleus in distinct energy levels.
c. Atoms consist of a small, massive, positively charged central portion
surrounded mainly by empty space where electrons orbited like planets.
d. Electrons occupy orbital clouds in complicated patterns around the positive
nucleus.
13. Which of the following correctly specifies the number of protons & electrons in an ion of scandium, Sc+3?
a. 45 p+, 48 eb. 21 p+, 18 ec. 45 p+, 42 ed. 21 p+, 24 e14. If you had a space suit coated with aluminum which type(s) of radiation would it be able to block or protect you from?
a. alpha
b. beta
c. gamma
d. both  & 
e. both  & 
15. What is the most radioactive of everyday examples listed below?
a. K of salt substitute, KCl.
c. Ra of old, glow in the dark clocks.
b. Am241 of smoke detectors.
d. C14 from your body.
16. How many orbital electron pairs are present in a sulfur atom?
a) 16
b) 8
c) 7
d) 9
17. The kernel of magnesium matches the electron configuration of which noble gas?
a) Kr
b) Ar
c) Ne
d) Xe
18. Which halogen is found in the same period as strontium?
19. (3pt Essay) What are the differences between the 2p and 4s sublevels?
20. (4 pts) Draw a picture of the neutral atom of C13 showing all of the protons, neutrons & electrons in the correct
locations and orbitals.
21. Carbon -14 has more _____ than carbon -12.
a. protons
b. neutrons
c. electrons
d. orbitals
22. The electron configuration of carbon is 1s22s22p2. How many energy levels and electrons are present?
23. (2 pts) Complete the following equation of radioactive decay for uranium.
238
beta
U -------------------->
92
24. An atom contains 43 protons, 45 neutrons, and 39 electrons. What is the symbol and charge of this ion?
a. Tc, +2
b. Rh, +6
c. Y, -3
d. Tc, +4
e. Rh, -2
25. An orbital represents the _____ space where a maximum of _____ can be found.
a. absolute, 1 proton
c. absolute, 1 electron
b. probable, 2 protons
d. probable, 2 electrons
26. What is an important outcome of Dimitri Mendeleev's work?
a. Charge Cloud Model
c. Plum Pudding Model
b. The Periodic Table
d. The Law of Definite Proportions
27. Flourine belongs to what family of elements?
a. Alkali Metals b. Transition Metals
c. Halogens
d. Noble Gases
28. A magnesium atom made up of 12 protons, 13 neutrons, and 12 electrons has a mass of
a. 37 u
b. 24 u
c. 25 u
d. 13 u
29. Which property of atoms decreases as you move to the right across the periodic table?
a. atomic radii b. ionization energy
c. electronegativity
d. density
30. Which type of radiation can cause damage to cellular molecules that may lead to cancer?
a. alpha
b. beta
c. gamma
d. delta
31. A 100 gram sample of Iodine 131 undergoes radioactive decay with a ½ life of 8 days. If the sample is left for 40 days,
what mass of I-131 will remain?
a. 20 g
b. 12.5 g
c. 6.25 g
d. 3.125 g
32. Nuclear power plants use uranium-235 as the primary fuel. What fission products are critical to maintain the chain
reaction?
a. bariums
b. kryptons
c. neutrons
d. positrons
33. Which family of elements are poor conductors, and react with metals to form salts due to their nearly complete octets in
the valence electrons?
a. noble gases
b. halogens
c. alkali metals d. metalloids
34. Which of the following properties of alkali metals is a chemical property?
a. react with water vigorously
c. soft
b. low melting points
d. low densities
35. Iron belongs to which family of elements?
a. halogens
b. semi-metals c. alkaline earth metals
d. transition metals
36. Which of the following is the complete electron configuration of chlorine?
a. 1s2,2s2,2p6,3s2,3p5
c. 1s2,2s6,2p2,3s2,3p5
2
2
5
b. 1s ,2s ,2p
d. 1s2,2s2,2p6,3s2,3p6,4s2,3d10,4p5
37. What element does the following abbreviated electron configuration correspond to?
[Ar]4s24p2
a. Si
b. Ca
c. Sn
d. Ge
38. Which of the following represents the greatest quantum leap?
a. 2s -> 3p
b. 1s -> 2s
c. 2s -> 3d
d. 3s -> 3p
39. (4 points) Obtain a piece of graph paper to
a. Carefully graph the following data.
b. Determine the half life of the isotope Ag112.
Time (min)
0
4
8
12
Mass (g)
11.8
7.3
4.7
3.2
16
2.1
20
1.0
24
.6
28
.4
40. If the atom C14 decays radioactively to produce a N14,
what kind of emission occurred?
a. alpha
c. gamma
14
d. delta
41. What are the valence electrons of Tin, Sn?
a) 4p2
b) 5s25p2
c) 3s23p6
d) 4s24p1
C
--?-->
6
14
N
7
e) 6s1
42. Why do atomic radii increase dramatically with each additional row of the periodic table?
a. atomic nuclei become increasingly attractive as more protons are added.
b. another energy level is utilized by the electrons.
c. the energy required to remove an electron is reduced by shielding of interior electrons.
d. relative sharing of electrons between atoms depends upon their electronegativity.
43. The elements of group 1A of the periodic table are called the
a. halogens
b. alkaline earth metals c. alkali metals d. noble gases
44. The electrons that are most responsible for an atom’s chemical behavior are called
a. kernel electrons
b. stable electrons
c. valence electrons
d. ionic electrons
45. Which block of the periodic table contains both metals and non-metals?
a. s-block
b. p-block
c. d-block
d. f-block
46. Which of the following elements will have the highest electronegativity in a covalent bond?
a. Na
b. Sc
c. As
d. Cl
47. Which of the following is the typical charge on the ions formed by alkaline earth metals?
a. 1b. 1+
c. 2d. 2+
48. Which of the following is not part of the noble gases?
a. xenon
b. neon
c. argon
Figure 5-1 Properties of X Group Elements
Element
Atomic Mass
Density (g/cm3)
(amu)
X
10
3
Y
4
Z
20
d. chlorine
Melting Point (oC)
200
300
Boiling Point (oC)
600
800
49. In Figure 5-1, what is the approximate atomic mass of element Y?
a. 5
b. 10
c. 15
d. 25
50. Imagine that a new element Q, of higher atomic mass than element Z in Figure 5-1 is discovered. If the density of the
new element is 6 g/cm3, where does it belong in the X group of elements?
a. above element X
b. between elements Y & Z.
c. below element Z
d. It does not belong in the X group.
Melting Point (oC)
Melting Point (oC)
of Alkali Metals
of Alkaline Earth Metals
2
180.5
1287
3
97.8
649
4
63.7
839
5
39.0
768
6
28.6
727
51. According to the table above, what element has a melting point of 180.5 oC?
a. hydrogen
b. cesium
c. beryllium
d. lithium
Period