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Periodic Table Book Assignment (Chapter 6)
Name ____________________________
1. List 3 properties of metals.
2. List 3 properties of nonmetals.
3. What are metalloids? Give 2 examples.
4. What are macronutrients? Give 3 examples.
5. What are trace elements? Give 3 examples.
6. Dimitri Mendeleev arranged the periodic table in order of increasing ___________.
7. Currently, the periodic table is arranged in order of increasing _____________.
8. What does the word “periodic” used in the periodic table of elements refer to?
9. Do elements in one family (vertical columns) or elements in one series (horizontal
rows) have the most similar characteristics in the periodic table? Explain.
10. Why does atomic radius decrease going across a row of the periodic table?
11. Why does atomic radius increase going down a column of the periodic table?
12. List 2 properties of the alkali metals.
13. List 2 properties of the alkali earth metals.
14. List 2 properties transition metals.
15. List 2 properties of the halogens.
16. Why are the noble gases so stable?
17. True or False: Elements in the same family have the same number of valence
electrons. Explain.
18. List 2 electrolytes that are essential to the central nervous systems in humans.
Atomic Structure Book Assignment (Chapter 5 – section 5.1 on pages 132-143)
1. What Greek philosopher proposed the idea of the atom? Did he support this idea
with experimental evidence?
2. Briefly describe (in your own words) the 4 pieces of Dalton’s atomic theory?
3. In what ways does our current model of the atom differ from Dalton’s model?
4. In 1897, J. J. Thomson discovered __________________
____________________ charged subatomic particles.
which are
5. What piece of equipment helped Thomson make this discovery?
6. In 1910, Ernest Rutherford performed his gold foil experiment. Based on this
experiment, summarize Rutherford conclusions about:
a. the composition of an atom’s nucleus
b. the size of a nucleus compared to the rest of an atom
7. Draw a picture of an atom. Identify the protons, neutrons, and electrons.
8. Are there subatomic particles that are even smaller than protons, neutrons, and
electrons?
9. Define atomic number.
10. What is atomic number of lithium?
11. Define isotope.
12. What are 2 isotopes of lithium that are naturally occurring (found in nature)?
13. Define mass number.
14. What is the mass number of lithium-7?
15. What is meant by electron cloud?
16. Opposite charges ___________________; like charges _________________________.
Periodic Table
Dimitri Mendeleev1. Listed the elements according to their atomic mass.
2. Noticed that similar chemical properties appeared at regular intervals.
3. Published first modern periodic table. Periodic Table of Elements.
Henry Moseley- Rearranged PT by atomic number
Periods: Horizontal rows on the periodic table. Represent how many energy levels each atom should
have. There are 7 periods.
Groups/Families: Vertical columns are called this because each group has similar properties because
they have the same number of electrons in the outer energy level. There are 18 groups.
Locations you should know
Metals: Solid at room temp., shiny, good conductors of heat and electricity, malleable (bendable),
ductile (made into wires), most can be corroded.
Nonmetals: Most are gases, some brittle and powdery solids, poor conductors of heat and electricity,
dull in appearance (not shiny).
Metalloids: Have properties of both metals and nonmetals. Next to zigzag line on the periodic table.
Metalloids often make up the semiconductors found in electronic devices.
Metalloids are B, Si, Ge, As, Sb, Te, At.
Alkali Metals: Group 1, like metals but HIGHLY REACTIVE. Soft, shiny, silver-white, good
conductors. Have one e- in their outer energy level which they like to give up. Never found
uncombined in nature. Reactivity increases down a group.
Alkali Earth Metals: Group 2, similar characteristics as alkali metals but not quite as reactive. They
have 2 electrons in the outer level which they like to give up. Never found uncombined in nature.
Transition Metals: Much less reactive than groups 1 and 2. They like to give up electrons – but the
number of electrons they give up can vary. Same properties as metals.
Halogens: Group 17 or 7A, need one more electron to obtain a stable outer energy level, reactivity
decreases as you move down period, gain electron(s) from a metal and form a salt compound. Most
reactive nonmetals, mostly gases.
Noble Gases: Group 18 or 8A, don’t usually react with other elements because they have a full outer
energy level. Also called “inert gases” because they are unreactive.
Rare Earth Elements:
1. Lanthanoid Series: Soft malleable metals with high luster and conductivity.
2. Actinoid Series: Radioactive elements made in the laboratory (synthetic).
Atomic Structure
Proton (p+): + charge, in nucleus, mass=1 amu
Neutron (n˚): Neutral charge, in nucleus, mass=1 amu
Electron (e-): - charge, floats outside nucleus in energy
levels, mass close to 0 amu (1/2000 the size of a proton)
Atoms are neutral (# of protons = # of electrons)
Atomic # = # of protons, identifies the element
Isotope: Atoms of the same element (same # of protons
and same # of electrons) that have different numbers of
neutrons. (Therefore, mass is different.)
Ex. Uranium-235 and Uranium-238, C-12 and C-14
Isotopes have identical chemical properties, but some
physical properties will be different.
Atomic Mass: Found on Periodic Table
Average mass of all the isotopes of that element as
they occur in nature.
Ex: Carbon’s atomic mass is 12.011. Are there more
atoms of carbon-12 or carbon-14?
Mass Number = # of protons + # of neutrons
OR
Rounded atomic mass (on periodic table)
Ex: Uranium-235 Atomic #=92, must be 143 neutrons
Uranium-238 Atomic #=92, must be 146 neutrons
Name
Hour
THE STRUCTURE OF THE ATOM
1. Complete the following chart:
Subatomic
Particle
proton
neutron
electron
Charge
Mass
(AMU)
Location
2. Important items to remember:
Atomic Number = # of _____________________
Mass Number = # of ________________ + _________________
Atoms are: a) Positive
b) Negative
c) Neutral
# of ________________ = # of ________________ in a neutral atom
3. Fill in the chart below:
ELEMENT
Symbol
Atomic
Number
# of
Protons
# of
Electrons
# of
Neutrons
SODIUM
MAGNESIUM
Mass
#
23
12
NITROGEN
14
ZINC
65
GOLD
LEAD
118
207
4. Explain what an isotope is and give an example:
Explanation:
Example:
5. Fill in the chart below:
Element
Symbol
Atomic #
# of p+
# of e-
# of n°
Carbon
C
6
6
6
6
Fluorine
Mass
Number
12
10
K
39
2
2
P
31
17
18
Copper
63
Copper
65
Sn
68
Sn
69
14
Al
Iron
28
14
56
6. There are 2 naturally occurring isotopes of copper. They are copper-63
and copper-65.
Which one is found in greater abundance?
How do you know this? (Hint: look at copper on your periodic table.)
Periodic Table Notes – Reactivity
Name ___________________
What combinations of elements can / cannot chemically react?
1.
Metals with Nonmetals (can react)
Form ionic compounds
Metals lose electrons
Nonmetals gain electrons
Examples:
2.
Nonmetals with Nonmetals (can react)
Form covalent compounds
Each nonmetal shares electrons
Examples:
3.
Metals with Metals (cannot react – but do form alloys which are mixtures)
4.
Special Case – Hydrogen (can react)
Hydrogen is versatile
Donates 1 electron
Examples:
Accepts 1 electron
Examples:
Shares 1 electron
Examples:
5.
Noble Gases (cannot react – some rare exceptions)
Reactivity Worksheet
Name ______________________
1.
Could the following elements react based on their position in the periodic table? If
so, would they form ionic or covalent compounds?
A)
calcium and bromine
H)
hydrogen and strontium
B)
nitrogen and iodine
I)
hydrogen and helium
C)
neon and lithium
J)
silicon and hydrogen
D)
cesium and barium
K)
phosphorus and hydrogen
E)
xenon and fluorine
L)
hydrogen and aluminum
F)
copper and zinc
M)
oxygen and potassium
G)
helium and hydrogen
N)
fluorine and carbon
2.
Could the following elements react based on their position in the periodic table? If
so, would they form ionic or covalent compounds?
A. Nitrogen and oxygen
I.
cesium and fluorine
B. Carbon and hydrogen
J.
chlorine and fluorine
C. Carbon and argon
K.
oxygen and krypton
D. Sodium and chlorine
L.
strontium and gold
E. Sodium and magnesium
M.
neon and helium
F. Tungsten and calcium
N.
bromine and magnesium
G. Copper and chlorine
O.
hydrogen and chlorine
H. Cesium and radium
P.
oxygen and carbon
Periodic Trends
1.
Name ______________________
Ionization Energy or IE (amount of energy needed to remove an electron from
an atom)
Across Table – IE increases because …
Down Table – IE decreases because…
2.
Atomic Size (radius)
Across Table – Size decreases because…
Down Table – Size increases because…
3.
Melting Points (MP) and Boiling Points (BP)
Metals usually higher than nonmetals
For metals: Down Table – MP/BP decrease because …
For nonmetals: Down Table – MP/BP increase because …
4.
Reactivity
Sides of table are more reactive (except for the noble gases)
For metals: Down Table – Reactivity increases because …
For nonmetals: Down Table – Reactivity decreases because …
Unit #3 – (Trends, Tables, and More)
Name ____________________
1.
Which of the elements in each lettered set has the lowest ionization energy?
Which has the highest ionization energy?
2.
3.
4.
A)
lithium
potassium
cesium
B)
lithium
boron
fluorine
C)
barium
calcium
arsenic
D)
argon
magnesium
potassium
Which of the elements in each lettered set is the smallest? Which is the largest?
A)
beryllium
carbon
fluorine
B)
lithium
sodium
potassium
C)
cesium
fluorine
neon
D)
calcium
rubidium
selenium
Which element in each lettered set has the lowest melting point? Which has the
highest melting point?
A)
lithium
potassium
cesium
B)
fluorine
chlorine
bromine
C)
strontium
calcium
bromine
D)
fluorine
chlorine
iron
Which element in each lettered set is most reactive? Which is least reactive?
A)
lithium
potassium
cesium
B)
fluorine
chlorine
bromine
C)
copper
zinc
potassium
D)
carbon
fluorine
neon
Atomic Models: Power Point Worksheet
Name ____________________
1. When did Democritus first propose the idea of the “atom”?
2. Give the 4 parts of Dalton’s atomic theory in your own words.
3. When was the electron discovered and by whom?
4. What is the approximate mass of the electron?
5. What device was used in the discovery of the electron?
6. Explain the model of the atom suggested by J.J. Thomson. (Include a diagram.)
7. Rutherford performed what experiment that helped define an atom?
8. What atomic structure did the above experiment help find?
9. Draw a diagram of the Rutherford experiment. Include labels.
10. Where do electrons go in the Bohr model of the atom?
11. What is the name of the Bohr atom?
12. How is the modern atom different from Bohr’s atom?
13. Who discovered the neutron?
14. What are quarks? What are their charges?
History of the Atom – Summary Activity
Directions - For each of the following scientists
a.
Describe their model of the atom
b.
Draw their representation of a lithium atom
c.
List the evidence they used to support their model
A. John Dalton
B. J. J. Thomson
C. Ernest Rutherford
D. Neils Bohr
E. James Chadwick