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 / B / C / D / E
/ / / /
  1. 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.
  1. I can name the three subatomic particles, their locations, & their charges in an atom.
Subatomic particle / Location / Mass / Charge
  1. I can use the periodic table to locate an element’s atomic mass & atomic number.
What subatomic particle determines what element an atom is? ______

  1. 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
  1. I can explain how atoms form ions.
  2. 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 / Atomic Number / Protons / Electrons / Charge
Cr+3
34 / 36
33 / -3
V+5
2 / 2
W+2
Show Lewis Dot diagrams of each atom and show movement/sharing of valence e-s.
Ionic :
aluminum bonds with chlorine / Covalent:
silicon bonds with oxygen
  1. I can write a chemical formulas and explain what it tells me about the compound.
Compound Name / Common Use / Chemical Formula / Name/ # of Elements / Total # of Atoms
calcium carbonate / chalkboard chalk / CaCO3
sodium phosphate / heavy-duty cleaner / Na3PO4
monosodium glutamate (MSG) / food seasoning / NaC5H8NO4
glucose / sugar / C6H12O6
freon-12 / refrigerator coolant / CCl2F2
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
  1. I can write a balanced chemical reaction.
____ KClO3 →____ KCl + ____ O2
____ H2O →____ H2 + ____ O2
____ KBr + ____FeI3→____ KI + ____ FeBr3 / ____ Zn + ____ HCl→____ ZnCl2 + ____ H2
____ Al + ____ Fe3N2→____ AlN + ____ Fe
____ CaO + ____ H2O →____ Ca(OH)2
___ 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.

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