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CHEMISTRY
TOPIC 1 SOL REVIEW HOMEWORK
Directions: Show all work where you see a * by either
explaining your answer or showing the mathematical set-up.
1. More than 2/3 of elements are a) metalloids
b) metals c) non-metals d) noble gases
2. The atomic number of a metalloid (semi-metal)
in Period 4 is a) 22 b) 33 c) 35 d) 72
3. Which of the following has the highest
ionization energy? a) Li b) Na c) K 4) Rb
4. Which of the following is most active?
a) neon b) boron b) beryllium c) lithium
5. Which of the following is the most active nonmetal? a) F b) Na c) Si d) Kr
6. Which of the following has the greatest tendency
to gain electrons? a) P b) C c) Cl d) B
7. Which of the following has the least tendency to
gain electrons? a) F b) I c) Br d) Cl
8. List two things that the elements listed in #7
have in common:
all are diatomics, all have 7 valence electrons, all
are halogens
9. The increase in atomic radius of each successive
element within a group is due to an increase in the
number of a) neutrons b) valence electrons
c) unpaired electrons d) principle energy levels
10. According to the modern periodic table, the
chemical properties of elements are a function of
their a) ionic charges b) oxidation states
c) atomic numbers d) mass numbers
11. Fill in blanks (high or low): Nonmetals have
_high_ionization energy and __low_electrical
conductivity
12. Circle one of the italicized words in each pair:
Metals tend to lose/gain electrons and become
positively/negatively charge while nonmetals tend to
lose/gain electrons and become
positively/negatively charged.
13. Which of the following is most likely to be
malleable? a) Au b) H2 c) S d) Rn
14. Elements in the same period all have the same
number of a) neutrons b) protons c) valence ed) occupied principle energy levels
15. Which of the following exhibits similar
properties? a) Mg, S b) Ca, Br c) Mg, Ca d) S, Cl
16. Which group contains elements whose atoms in
the ground state have a total of five electrons in
their outermost p sublevel? a) noble gases
b) halogens c) transition metals d) alkali metals
17. Which group contains elements with four
electrons in the outermost principle energy level?
a) group 1 b) group 14 c) group 16 d) group 18
18*. Which is the electron configuration of a
transition metal? a) 1s22s2
b) 1s22s22p63s2 c)
1s22s22p63s23p6
d) 1s22s23s23p64s23d1
19. How many valence electrons does the following
electron configuration have? 1s22s22p63s23p4 six
20. How do the masses of Cl and Cl- compare? they
are the same
21. Which diagram represents an atom of fluorine
in an excited state? a) ↑↓ ↑↓ ↑↓ ↑↓ ↑_
b) ↑↓ ↑_ ↑↓ ↑↓ ↑↓ c) ↑↓ ↑↓ ↑↓ ↑↓ ↑↓
d) ↑↓ ↑↓ ↑↓ ↑↓ ↑_ ↑_
22. The s sublevel has __1_ orbital(s).
23. An atom of 226Rn has _86__ protons,
86
_86__ electrons and _140_ neutrons
24. Compared to an atom of 12C, an atom of 14C has
a) more protons b) less protons c) more neutrons
d) less neutrons
25. How are the bright-line spectrum of elements
produced? when electrons go from a higher energy
level back to the ground state releaseing enegy in
the form of visible light
26. When at atom goes from the excited state to the
ground state, the total energy of the atom
____decreased____
27. The kernel usually includes parts of the atom
except the a) neutrons b) protons c) orbital
electrons d) valence electrons
28. The amount of energy required to remove the
most loosely bound electron from an atom in the
gaseous phase is called a) kinetic energy b)
potential energy c) ionization energy d) eaffinity
29. Which two particles have approximately the
same mass? a) neutron and electron b) neutron
and deuteron c) proton and neutron d) proton
and electron
30. Indicate the number of valence electrons:
a) Fr 1
b) 1s22s23s23p64s23d104p4 6
c) Cl 7
d) Cl- 8
e) He 2
f) any noble gas other than He 8
g) ↑↓ ↑↓ ↑↓ ↑↓ ↑_ 7
h) Al 3
i) Al3+ 8