U9 Matter Test Review WS 2015
1. I can describe the important models of the atom leading to the modern theory.
 Label each model with the name of the scientist who “discovered” the model and the main
feature of the model. (Bohr, Democritus, Rutherford, Dalton, Schrodinger)
A
2.
B
C
D
E
I can define the terms atomic mass and atomic number.
 What part of the atom accounts for the majority of the atom’s mass?
 What part of the atom accounts for the majority of the atom’s volume?
 What does the atomic number of an atom tell you?
 What does the mass number of an atom tell you?
 Atoms are _______________, or have no total charge, because the number of __________
and ___________ in the atom are equal.
 _____________ are atoms of the same element that have different numbers of neutrons.
 ___________ is a charged atom formed by the loss or gain of an electron.
3.
I can name the three subatomic particles, their locations, & their charges in an atom.
Subatomic particle
4.
Location
Mass
Charge
I can use the periodic table to locate an element’s atomic mass & atomic number.

What subatomic particle
determines what element an atom is?
____________
5.
I can use the periodic table to show that elements are organized based upon repeating patterns of
physical and chemical properties
 Complete the table below.
group #
1
2
13
14
15
16
17
18
# valence
electrons
expected
charge
6. I can explain how atoms form ions.
7. I can explain how valence electrons are involved in chemical compounds formation.
 what is an ion? ____________________________________________
 cation: charge? _____ gain or lose e-s? ________ metal or non-metal? ________
 anion: charge? _____ gain or lose e-s? ________ metal or non-metal? ________
 ionic bond: steal or share e-s? ____________________
 covalent bond: steal or share e-s? ____________________
 ionic compound: types of elements? ________________ type of bonds? __________
 molecular compound: types of elements? ________________ type of bonds? __________
 Complete the table below.
Ion Symbol
Cr
Atomic Number
Protons
Electrons
Charge
+3
34
36
33
-3
V+5
2
W+2
2
Show Lewis Dot diagrams of each atom and show movement/sharing of valence e-s.
Ionic :
Covalent:
aluminum bonds with chlorine
silicon bonds with oxygen
8.
I can write a chemical formulas and explain what it tells me about the compound.
Compound Name
Common Use
Chemical Formula
calcium carbonate
chalkboard chalk
CaCO3
sodium phosphate
heavy-duty
cleaner
food seasoning
Na3PO4
NaC5H8NO4
sugar
C6H12O6
refrigerator
coolant
CCl2F2
monosodium
glutamate (MSG)
glucose
freon-12
Name/ # of
Elements
Total # of
Atoms
 Ionic Compounds: Write names on right and write formulas on left.
1. Na2O ________________
5. potassium iodide ________________
2. Mg3N2 ________________
6. magnesium oxide ________________
3. K2S ________________
7. calcium sulfide ________________
4. Li3P ________________
8. aluminum chloride ________________
 Molecular Compounds: Write names on right and write formulas on left.
1. CO2 ________________
5. boron trichloride ________________
2. NH3 ________________
6. sulfur hexafluoride ________________
3. CF4 ________________
7. iodine trichloride ________________
4. SiO2 ________________
8. nitrogen dioxide ________________
 Ionic or Molecular Compounds: ionic compound or a molecular compound? Explain.
1. PCl5
2. MnO2
3. Mg3N2
4. IBr3
9.
I can write a balanced chemical reaction.
____ KClO3
____ Zn + ____ HCl → ____ ZnCl2 + ____ H2
→ ____ KCl + ____ O2
____ Al + ____ Fe3N2 → ____ AlN + ____ Fe
____ H2O → ____ H2 + ____ O2
____ CaO + ____ H2O → ____ Ca(OH)2
____ KBr + ____FeI3 → ____ KI + ____ FeBr3
___ Cu + ___ Ag(NO3) → ____Cu(NO3)2 + ___ Ag
Vocabulary:
_____ 1.
atomic number
_____ 2.
periodic table
_____ 3.
mass number
_____ 4.
group
_____ 5.
isotope
_____ 6.
atomic mass unit (amu)
_____ 7.
atomic mass
_____ 8.
period
_____ 9.
electrons
_____ 10.
protons
_____ 11.
neutrons
_____ 12.
nucleus
_____ 13.
atom
_____ 14.
John Dalton
_____ 15.
Democritus
_____ 16.
J.J. Thompson
_____ 17.
ion
_____ 18.
formula
_____ 19.
valence electron
_____ 20.
Bohr
A. atoms that have the same number of protons but
different numbers of neutrons
B. weighted average mass of the atoms in a naturally
occurring sample of an element
C. equals the number of neutrons plus the number of
protons in an atom
D. 1/12 the mass of a carbon-12 atom
E. the number of protons in the nucleus of an atom of an
element
F. an arrangement of elements according to similarities in
their properties
G. a vertical column of elements in the periodic table
H. a horizontal row of the periodic table
I. the central core of an atom, which is composed of
protons and neutrons
J. negatively charged subatomic particles
K. subatomic particles with no charge
L. positively charged subatomic particles
M. Greek philosopher who was among the first to suggest
the existence of atoms
N. the smallest particle of an element that retains its
identity in a chemical reaction
O. English chemist and schoolteacher who formulated a
theory to describe the structure and chemical
reactivity of matter in terms of atoms
P. Danish scientist who proposed that electrons orbit
around nucleus in defined energy levels.
Q. electron(s) in outermost energy level
R. symbolic representation of elements and number of
atoms in a molecule.
S. atom with a charge due to loss/gain of electrons.
T. English scientist who proposed that mobile negatively
charged electrons were embedded in a positive atom.
U. Greek scientist who named the atom as the smallest,
indivisible particle of matter.
V. English scientist who proposed that atoms could
combine to form compounds.
Fill in the table below: