CHAPTER 4 QUIZ II NAME______________________
CHAPTER 4 test ATOMIC STRUCTURE NAME____________________
1. List five of the six parts to Dalton’s atomic theory.
2. Of Mr. Dalton’s statements, which was proven to be false and why?
3. What were the major points of Aristotle’s theory?
4. What were the major points of Democritus’ theory?
5. Define atom.
6. By each statement, write either proton, neutron, and/or electron. If more than one apply, you must put down all that apply!
a)____________ discovered by Rutherford b)________________ discovered by Chadwick
c)____________ relative mass of zero d)________________ relative mass of 1
e)____________ real mass of 9.1x10-28g f)________________ positively charged
g)____________ real mass of 1.7x10-24g h)________________ found outside the nucleus
i)_____________ neutral j)_________________ found inside the nucleus
k)____________ make up all the space l)_________________ make up all the weight
of an atom of an atom
m)____________ mass number is the total n)________________ atomic number represents
number of these the amount of these
o) _____________ negatively charged
7. What is the world’s population? How many atoms could each person in the world get from one penny?
8. What is the plum pudding model? Whose idea was it?
9. Describe a cathode ray tube. What common devices use them?
10. For this nuclide: Br1- -80
a) how many protons are there?__________
b) how many electrons are there?__________
c) how many neutrons are there?__________
d) what does Z equal?________
e) what does A equal?_________
11. For this nuclide: Ra2+-225
a) how many protons?_________
b) how many electrons?________
c) how many neutrons?________
d) what does Z equal?_________
e) what does A equal?_________
12. Name two subatomic particles.
13. Calculate the average atomic mass of an element with these relative amounts:
2.62% is 78.976 u 23.11% is 82.956 u 56.90% is 83.912 u 17.37% is 85.911 u
What elements is this most likely to be?
14. Complete this table:
protons neutrons electrons mass number atomic number
As-75
53 127
16 17 18
209Po2- 84
[pic]
36 88 38
15. Define each:
a. Cathode
b. Alpha particle
c. Gamma rays
d. Nuclide
e. Mass number
f. Atomic mass
g. Atomic number
h. Half life
i. tritium
14. Describe the gold foil experiment and the conclusions made from it (3pts)
15. Describe how carbon dating works. (4 pts)
16. List the names of the three isotopes of hydrogen. How many protons, electrons, and neutrons are in each? Which is most common? How do you know? (5pts)
17. Write the equation for the alpha particle decay of a radium-226 atom. Write the equation for the beta decay of thorium-234. (6pts)
Multiple choice
1. Which of the following statements from Dalton's atomic theory is no longer true, according to modern atomic theory?
A) Elements are made up of tiny particles called atoms.
B) Atoms are not created or destroyed in chemical reactions.
C) All atoms of a given element are identical.
D) Atoms are indivisible in chemical reactions.
E) All of these statements are true according to modern atomic theory.
2. The Greeks proposed that matter consisted of four fundamental substances:
A) fire, earth, water, air
B) fire, metal, water, air
C) earth, metal, water, air
D) atoms, fire, water, air
E) atoms, metal, fire, air
3. The first scientist to show that atoms emit any negative particles was
A) J. J. Thomson.
B) Lord Kelvin.
C) Ernest Rutherford.
D) William Thomson.
E) John Dalton.
4. The scientist whose alpha-particle scattering experiment led him to conclude that the nucleus of an atom contains a dense center of positive charge is
A) J. J. Thomson.
B) Lord Kelvin.
C) Ernest Rutherford.
D) William Thomson.
E) John Dalton.
5. If the Thomson model of the atom had been correct, Rutherford would have observed
A) alpha particles going through the foil with little or no deflection.
B) alpha particles greatly deflected by the metal foil.
C) alpha particles bouncing off the foil.
D) positive particles formed in the foil.
E) None of these observations is consistent with the Thomson model of the atom.
6. Rutherford's experiment was important because it showed that:
A) radioactive elements give off alpha particles.
B) gold foil can be made to be only a few atoms thick.
C) a zinc sulfide screen scintillates when struck by a charged particle.
D) the mass of the atom is uniformly distributed throughout the atom.
E) an atom is mostly empty space.
7. Which of the following atomic symbols is incorrect?
A) [pic]
B) [pic]
C) [pic]
D) [pic]
E) [pic]
8. The element rhenium (Re) exists as two stable isotopes and 18 unstable isotopes. Rhenium-185 has in its nucleus
A) 75 protons, 75 neutrons.
B) 75 protons, 130 neutrons.
C) 130 protons, 75 neutrons.
D) 75 protons, 110 neutrons.
E) not enough information is given.
9. [pic] has
A) 20 protons, 20 neutrons, and 18 electrons.
B) 22 protons, 20 neutrons, and 20 electrons.
C) 20 protons, 22 neutrons, and 18 electrons.
D) 22 protons, 18 neutrons, and 18 electrons.
E) 20 protons, 20 neutrons, and 22 electrons.
10. Which of the following has 45 neutrons, 35 protons, and 36 electrons?
A) [pic]
B) [pic]
C) [pic]
D) [pic]
E) [pic]
11. The numbers of protons, neutrons, and electrons in [pic] are:
A) 52 p, 128 n, 53 e
B) 53 p, 127 n, 54 e
C) 53 p, 127 n, 52 e
D) 53 p, 74 n, 54 e
E) 53 p, 74 n, 52 e
12. All of the following are true except:
A) Ions are formed by adding electrons to a neutral atom.
B) Ions are formed by changing the number of protons in an atom's nucleus.
C) Ions are formed by removing electrons from a neutral atom.
D) An ion has a positive or negative charge.
E) Metals tend to form positive ions.
13. By knowing the number of protons a neutral atom has, you should be able to determine
A) the number of neutrons in the neutral atom.
B) the number of electrons in the neutral atom.
C) the name of the atom.
D) two of the above.
E) none of the above
14. An ion is formed
A) by either adding or subtracting protons from the atom.
B) by either adding or subtracting electrons from the atom.
C) by either adding or subtracting neutrons from the atom.
D) All of the above are true.
E) Two of the above are true.
15. An isotope, X, of a particular element has an atomic number of 7 and a mass number of 15. Therefore,
A) X is an isotope of nitrogen.
B) X has 8 neutrons per atom.
C) X has an atomic mass of 14.0067.
D) X is an isotope of nitrogen and X has 8 neutrons per atom.
E) X is an isotope of nitrogen, X has 8 neutrons per atom, and X has an atomic mass of 14.0067.
16. A species with 12 protons and 10 electrons is
A) Ne2+
B) Ti2+
C) Mg2+
D) Mg
E) Ne2–
True or False: IF FALSE, REPLACE THE WRONG PART WITH A CORRECT PART
1. The modern periodic table is arranged by increasing atomic mass of the elements.
2. Aristotle named atoms atoms.
3. A cathode ray tube consists of a stream of protons.
4. In a neutral atom, the number of protons is equal to the number of neutrons.
5. Gamma decay emits energy but no particles.
6. An alpha particle is the equivalent of a Helium-4 nucleus.
7. Nuclear decay can change one element into another one.
8. Isotopes are forms of an element that have the same number of protons but a different number of electrons.
9. An input of energy is required in order for nuclear decay to happen in an atom.
10. Gamma decay is a form of nuclear radiation that consists entirely of energy, not matter.
11. The stability of a nucleus is determined by the ratio of electrons to protons.
12. The mass of a neutron is approximately equal to the mass of a proton.
13. The modern periodic table is arranged from right to left in order of increasing atomic mass.
14. Greek philosophers thought that matter was composed of four elements: air, earth, fire, and water.
15. In the notation [pic], 107 represents the atomic number and 47 represents the atomic mass of silver.
16. Radon is a radioactive substance that undergoes spontaneous emission of radiation due to its unstable nuclei.
17. Atoms of a radioactive element can change into atoms of another element by emitting radiation.
18. A proton is a subatomic particle carrying a charge equal to but opposite that of an electron.
19. Cathode rays are deflected toward a negatively charged plate in an electric field.
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