Final Exam Vocabulary Review:
Chemical symbol
Atom
ion
Proton
Neutron
Electron
Atomic number
Electron cloud
Energy level
Atomic mass (mass number)
Average atomic mass
Isotope
Periodic table
Dimitri Mendeleev
Compound(s)
Chemical formula
Charge (oxidation number)
Valence electron
subscript number
chemically stable
chemical bond
superscript number
ionic bond
covalent bond
binary compound
polyatomic ion
Questions:
1. For each of the seven scientists listed below, give an explanation of their
contribution to atomic theory, a description of their experiment (Thomson and
Rutherford), and a diagramed model of their atom.
Democritus:
Dalton:
Thomson:
Rutherford
Bohr
Chadwick
Modern Atomic Model (Electron Cloud)
2.
How are isotopes of the same element alike and how are they different?
3.
How are ions formed?
4. What is the difference in structure between a positive ion and a negative ion?
5. What are the names and charges of particles found within the atom? Identify (by
drawing) the location of these particles.
6. Compare and contrast Thomson’s plum pudding model with Rutherford’s nuclear
atomic model.
7. Compare and contrast Bohr’s energy level diagram with the Modern Atomic Model.
8. Which statement(s) is (are) consistent with Rutherford’s gold foil experiment?
a.
b.
c.
d.
all atoms have a positive charge
all atoms are mostly empty space
the nucleus of the atom contains protons and electrons
mass is spread uniformly throughout the atom.
9. Which subatomic particle determines the identity of the atom? Where is it found
in the atom? How is this particle related to the element’s atomic number?
10. Which subatomic particles account for the majority of mass of the atom? Where
are they located?
Element
(atom name)
Atomic
number
20
Atomic
mass
40
39
13
12
58
6
carbon
Protons
Neutrons
20
22
electrons
20
26
5
8
The elements represented in rows 1, 2, and 3 in this table are called isotopes because
__________________________________________________________________.
11. Which of the following are isotopes:
a.
12
6C
and
12
6
b.
12
6C
and
13 C
6
c.
12
6C
and
13 N
7
C
12. What is the atomic mass of hafnium if, out of every 200 atoms, 10 atoms have a
mass of 176, 38 atoms have a mass of 177, 54 atoms have a mass of 178, 28 atoms
have a mass of 179, and 70 atoms have a mass of 180.
13. Eighty percent of the isotopes of iodine have a mass of 127, seventeen percent
have a mass of 126, and three percent have a mass of 128. What is the average
atomic mass of iodine.
14. Calculate the average atomic mass of iridium using the following data: iridium
191 has a natural abundance of 37.58% and iridium 193 has a natural abundance of
62.42%.
15. Here are three isotopes of an element.
7
14
N
7 N
15
7 N
16
The element is __________________
The number 7 refers to _____________
The numbers 14, 15, and 16 refer to ___________________
How many protons and neutrons are in the first isotope ____________________
How many protons and neutrons are in the second isotope __________________
How many protons and neutrons are in the third isotope__________________
16. Identify the following elements:
98?
43
75?
_____________
33__________
17. Atom A has 5 protons and 6 neutrons, Atom B has 6 protons and 5 neutrons,
these atoms are _____________________________________________________.
18. Isotopes always have the ______________ but different ___________________.
19. Strontium has four stable isotopes, Strontium - 84 has a very low natural
abundance, but 86Sr, 87Sr, and 88Sr are all reasonably abundant. Which of these
abundant isotopes predominates?
20. How many valence (outer shell) electrons do each of the following elements have?
Be ______
F ______
He ______
Al ______
S_______
Mg ____
21. Is it likely that the charge shown will form?
N3- __________
Li1+__________
O2-________
Mg2-__________
22. Explain why Lithium is a reactive element while Helium is not.
23. Why does Magnesium loses electrons to form bonds, while oxygen gains
electrons?
24. Draw Bohr diagrams (electron arrangements) for the following atoms:
Helium
Nitrogen
Aluminum
Calcium
25. Diagram each atom with the correct number of valence electrons. Will the
following atoms bond together? Will the bond be ionic or covalent? Explain your
answer.
Be
+
O
Be2+
+
O2-
F
Si
+
F + F + F + F
F
Si F
F
Na
+ I
+ I
Na
1+
+
I
1-
+
I1-
26. Determine the identity of each element in the formula, the number of atoms of
each element, and the total number of atoms in the formula:
Ba(OH)2
3 (NH4)2SO3
Ca3(PO4)2
27. Complete the following chart:
Chemical Element Atomic Atomic Number Number Number charge Atom
symbol
number mass
of
of
of
or
protons neutrons electrons
ion?
26
IRON
Cl
34
58
24
37
18
2
4
34
80
atom
2-
Cr
28
47
3+
ion
21
108
1+
29. Write the chemical formulas for each of the compounds in the box:
chloride
phosphate
sulfide
sulfate
arsenate
magnesium
Iron (II)
silver
Platinum (IV)
Gold (III)
Write correct molecular formula for the following:
Chlorine monoxide __________________________________
Dinitrogen trioxide _________________________________
Triboron nonahydride _______________________________
Tetraphosphorus decasulfide ________________________
Iodine heptafluoride ________________________________
Please review all formula writing and naming notes and worksheets. Since we have
recently completed these I have not focused the review on them. They will be a
considerable part of your final exam.