1st Quarter Benchmark Study Guide 2010/2011 Name_____________Date __ Period__
In addition to the questions below, you need to know all the definitions on the 1st
Nine Week AKS Checklist at the back of this study guide. Many are imbedded in the questions
below.
1. What is matter? What two properties does all
matter have?
Bohr Model of Sodium
2. Draw a Sodium atom using a Bohr Model.
a. label its parts (include the nucleus)
b. Label the charges on each subatomic
particle (proton, neutron, electron)
c. Show what its charge would be if ionized.
d. Forms a cation or anion?
e. Show the Lewis Dot model
3. Draw an Oxygen atom using a Bohr Model
a. label its parts (include the nucleus)
b. Label the charges on each subatomic
particle (proton, neutron, electron)
c. Show what its charge would be if ionized.
d. Forms a cation or anion?
e. Show the Lewis Dot model
Lewis Dot .
Bohr Model of Oxygen
Lewis Dot
4. What are valence electrons? Why are these subatomic particles so important? For some
elements, what is a quick way to determine the number of valence electrons that it has?
5. Identify the following:
a. Element symbol
b. Number of protons
c. Number of electrons
d. Mass
e. Number of neutrons (how do you know this?)
34
Se
79
6. The Periodic Table is arranged by increasing ____________ _________________ and by
the __________________ of the elements.
7. The vertical (up/down) columns of the Periodic Table (PT) are called _____________ or
_________________. Elements in these groups have ______________ physical and
chemical _________________.
8. The horizontal (right to left) rows are called _______________.
9. _______________ are on the left side of the Periodic table and ______________ are
on the right side of the Periodic Table. _________________ are on the zigzag line.
10. This number represents the number of ______________ in each element on the Periodic
Table.
11. Label ALL of the trends on the periodic table below: increasing atomic number,
increasing atomic mass, decreasing reactivity, increasing reactivity (from zigzag line).
Color the metals yellow, nonmetals blue and metalloids green. Label the different family
groups: alkaline metals, alkaline earth metals, transition metals, halogens, noble gases.
12.
In an atom, the number of _____________ will be the same as the number of
__________________.
13. Describe 5 characteristics of metals.
14. Describe 5 characteristics of nonmetals.
15. Describe 4 characteristics of metalloids. Name the metalloid elements.
16. What is the difference between a physical and chemical property?
17. What is volume?
18. What is mass?
19. What is density? What is the equation for density?
Calculate the density of a cube that has a side measure of 3 cm and a mass of 27 grams.
(Remember, the volume for a cube is V = l x w x h or V = s 3 . Remember the units!)
Which substance has a higher density? Benzene has a mass of 4.40 g for a 5 ml sample
Toluene has a mass of 4.35 g for a 5 ml sample
20. Pick one object (a car, pencil, book etc). Name the object and give two examples of a
chemical property as well as five examples of a physical property.
21. What is the difference between a physical and chemical change? What is another name
for a chemical change?
22. Give two examples of a physical change.
23. Give two examples of a chemical change and state the one condition that must be met to
ensure that the change was a chemical one.
24. Phase changes (changes from solids to liquids or gases) are ____________ changes.
25. List all the phase changes of water and tell what phase is becoming what new phase and
if energy is added or removed.
26. Draw models of a solid, liquid and a gas showing the arrangement of particles. Describe
the movement of the particles in each.
Solid:
Liquid:
Gas:
Movement:
Movement:
Movement:
27. What phase change involves a substance going from the solid phase directly to the gas
phase?
What is the reverse called?
28. Label these changes as physical or
chemical.
a. digesting of food
b. explosion
c. acid rain
d. ice cube melting
e. crushing rocks
f. lighting a candle
g. water boiling
h. sugar dissolving in tea
29. Label these properties as physical or
chemical.
a. ductility
b. texture
c. melting point
d. density
e. malleability
f. tendency to rust/corrode
g. volume
h. flammability/combustibility
30. What two types of substances are pure substances? Why are these classified as a pure
substance?
31. What is a compound? What is the smallest particle of a compound?
32. How many elements are included in NaHCO3? _____How many atoms?____ (list the elements
as well as the number of atoms of each). What is ‘NaHCO3’ called?
33. This is the structural model of a molecule of sucrose, a type of
sugar. The chemical formula is C12H22O11. What different elements
make up sucrose and how many atoms of each are in the compound?
34. How can a person identify a mixture?
35. Fill in the chart below.
Substance
Definition (made of
what type of particle)
How are the combined?
(type of change –
physical or chemical)
How are they
separated?
Element
Compound
Mixture
36. What are the different types of heterogeneous and homogeneous mixtures? (see vocabulary
for chapter 4)
37. Draw a picture showing models of the following:
a. a molecule of one type of element (this will be a diatomic molecule)
b. a molecule of two different elements (what is another name for this?)
c. a mixture made of one type of element and one type of compound
d. a mixture made of two different types of compounds
a
b
c
38. How is an atom different from a molecule?
39. What does the Law of Conservation of Matter say? Explain!
d
40. New substances are formed as a result of chemical reactions (a chemical change). The
chemical reaction shown below shows what happens when natural gas (ethane, or C2H6) is
burned (combining with the oxygen in the air) giving off carbon dioxide and water (or in
this case steam). Identify the reactants, the products and prove that the Law of
Conservation of Mass is true by counting atoms of each element on each side and balancing
the equation.
___ C2H6 + 7 O2
___ CO2 + 6 H2O
41. You combine 2 compounds together in a baggie with an activator. Before the reaction
occurred, the mass was 36.1 grams. After the reaction is complete, what should the mass
of your products be? __________ This demonstrates what?_______________________
42. When a gas moves into a plasma state, what has happened to the energy of the
particles?
43. Compared to the gas state, how are the particles moving?
44. What is the transition called from gas to plasma? ________________ From plasma to
gas? _________________
45. Why does the temperature of a substance remain the same during the process of
transition from solid to liquid?
46. Label the 4 parts of this equation: 2H + 2O
2H2O
47. Who is usually given credit for using the word: “atom”
48. What were the 4 elements, according to ancient Greek philosopher?
49. Who began the modern atomic theory?
50. Which two scientists developed and refined the modern periodic table?
51. Who discovered the electron?
52. What 4 factors (collision theory) influence the rate of chemical reactions and how?
53.
54.
55.
56.
Increased temperature means greater average energy of ______________.
What does “kinetic” mean?
When strong acids and strong bases combine, they produce _____________.
The pH scale is a measurement of :
57. Describe the range of the pH scale and what type of substances can be found at each
end and in the middle of it.
58. Why are elements in period 1 the most reactive?
Indicators of Achievement:
11a - distinguish between atoms and molecules
____ differentiate between protons, neutrons,
electrons by mass, charge,
location and function (role)
____ draw atomic structure of an element given
number of protons, atomic
mass and charge
____ Extension: define and recognize isotopes
____ define and determine number of valence
electrons for element
____ define molecule
11b - describe the difference between pure
substances (elements and
compounds) and mixtures
____ define element
____ define compound
____ write chemical formulas for common
compounds
____ define pure substance
____ define mixture (homogeneous, heterogeneous)
____ define solution, solvent, solution
____ differentiate between homogeneous and
heterogeneous mixtures
____ differentiate between elemental molecules and
molecules of
compounds
____ draw particle examples of elements,
compounds, pure substances and
mixtures
____ classify substances as an element, compound,
pure substance or
mixture
11c - describe the movement of particles in solids,
liquids, gases and
plasma states
____ define solid, liquid, gas and plasma
____ differentiate between solids, liquids and gases
in terms of shape and
volume
____ compare the motion of particles in solid, liquid,
gas and plasma
____ compare the arrangement of particles in solid,
liquid, gas and plasma
11d - distinguish between physical (density, melting
point, boiling point) and
chemical properties of matter (reactivity,
combustibility)
____ define and recognize physical properties such
as mass, volume,
density, weight, state (s/l/g), size, shape,
color, texture, odor,
hardness, freezing/melting/boiling points, etc
____ define and recognize chemical properties such
as reactivity
(corrosiveness), flammability, combustibility
____ understand density and know how to calculate
(mass/volume)
11e - distinguish between physical and chemical
changes (development of a
gas, formation of a precipitate and/or change
in color) in matter
____define and recognize physical changes (changes
only the way in which
existing substances are organized) such as
phase change (melting
and freezing, boiling and condensing),
dissolving and coming out of
solution, forming a mixture, etc
____ 11g - Extension: analyze energy transfer
associated with phase
change (energy vs temperature graph)
____ define and recognize chemical change
(changes in how atoms are
bonded together). A chemical change results
in the creation of new
substance(s) and/or the destruction of
existing substance(s).
11f - identify and demonstrate the Law of
Conservation of Matter
____ state the Law of Conservation of Matter
____ recognize examples of conservation of matter
____ Extension: 12e – balance simple chemical
equations (single
replacement and synthesis reactions)
12a - use the Periodic Table of Elements to gather
information about an
element
____ using an entry in the periodic table, determine
an element’s name,
chemical symbol, atomic number, atomic
mass, standard state and
number of valence electrons (groups 1, 2, 13
– 18)
12b - classify elements as metals, nonmetals or
metalloids using the
periodic table
____ based on location in the periodic table, classify
as element as metal,
non-metal or metalloid
____ differentiate between metals, non-metals and
metalloids as to luster,
ductility, malleability, hardness, electrical and
thermal conductivity,
standard state, valence electrons, and
reactivity
12c - use the periodic table to explain the similarities
and differences
between elements
____ explain the arrangement/organization of the
periodic table
____ define groups or families
____ state key characteristics of different families in
periodic table
____ define periods
12d - identify common chemical symbols, formulas
(i.e., H2O, NaCl, H2SO4)
____ state chemical name based on chemical
symbols for elements
____ state chemical name based on chemical
formula for common
compounds
12e - Extension: balance simple chemical equations
such as single
replacement and synthesis reactions
Vocabulary:
(Check off the ones that you know and look up the ones that you don’t know!)
atom
physical property
nucleus
mass
proton
volume
neutron
density
electron
weight
electron cloud
physical change
valence electron
phase change
isotope
melting point
element
boiling point
molecule
evaporate
periodic table
condense
chemical symbol
freezing point
chemical name
solid
atomic number
liquid
atomic mass
gas
groups
plasma
families
chemical property
metals
reactivity
non-metals
combustibility
metalloids
flammability
luster
chemical change
malleability
precipitate
ductility
conductivity
noble gases
compound
pure substance
mixture
solution (soln)
solvent
solute
homogeneous solution
heterogeneous solution