Look at a periodic table to answer the following questions:
1.
2.
3.
4.
5.
6.
7.
What is the name of group 1?
What is the name of group 2?
What is the name of group 17?
What is the name of group 18?
What is the name for the d block?
What is the name for the s & p block?
What is the name for the 2 periods at the bottom of the periodic table?
Answer the following questions with these terms:
Noble gases
Transition metals
Halogens
Alkali metals
Alkaline-earth metals
8. The _____________________ have a single electron in the highest energy level?
9. The _____________________ achieve the electron configurations of noble gases by
losing two electrons.
10. The _____________________ vary in the number of electrons in the highest energy
level.
11. The _____________________ achieve the electron configurations of noble gases by
gaining one electron.
12. The _____________________ have full s and p orbitals in the highest occupied energy
levels.
13. The _____________________ are stable and unreactive.
14. The _____________________ are highly reactive and readily form salts with metals.
15. The _____________________ are metals that are more reactive than the transition
elements but less reactive than the alkali metals.
3
Li
Lithium
6.94
11
Na
Sodium
22.989
4
Be
Beryllium
9.0121
12
Mg
Magnesium
24.305
16. Which element will react more readily with
chlorine: sodium or magnesium? Why?
17. Which element is more like lithium in terms of
properties: sodium or beryllium? Why?
18. Which element has more electrons in its highest
occupied energy level: sodium or magnesium?
19. Which element has a lower melting point: lithium or beryllium?
20. Which element is closer to achieving noble gas configuration: magnesium or lithium?
21. Which element reacts more readily with fluorine: lithium or beryllium? Why?
For each choice of words, circle the one that best completes the sentence.
1. The shielding effect increases with increasing atomic number within a (period, group).
2. In any (period, group), the number of electrons between the nucleus and the outer energy
level is the same.
3. Within a group, the nucleus has a stronger ability to pull on the outermost electrons in
elements of (high, low) atomic number.
4. The more (positive, negative) the value of electron affinity is, the more easily the atom
can take on an extra electron.
5. From left to right across a period, electron affinity values become more (positive,
negative).
6. The halogens have the (most, least) negative electron affinity values.
7. The (electronegativity, electron affinity) of an atom is the tendency of an atom to attract
electrons to itself when it is chemically combined with another element.
8. The (noble gases, halogens) are the most electronegative group.
Use the following choices:
a. increases
b. decreases
c. remains constant
d. there is no pattern
9. Moving from top to bottom in a group, atomic radius tends to _____________.
10. Moving from top to bottom in a group, shielding effect tends to _____________.
11. Moving from top to bottom in a group, electronegativity tends to _____________.
12. Moving from top to bottom in a group, electron affinity tends to _____________.
13. Moving from top to bottom in a group, ionization energy tends to _____________.
14. Moving from left to right across a period, atomic radius tends to _____________.
15. Moving from left to right across a period, shielding effect tends to _____________.
16. Moving from left to right across a period, electronegativity tends to _____________.
17. Moving from left to right across a period, electron affinity tends to _____________.
18. Moving from left to right across a period, ionization energy tends to _____________.
19. Which atom has the more negative value for electron affinity, sodium or chlorine?
20. Which atom is more electronegative, fluorine or lithium?
21. Which atom has a greater ionization energy, nitrogen or bismuth?
22. Which atom exerts a stronger pull on its outermost electrons: calcium or arsenic?
23. Which atom has a larger atomic radius, fluorine or barium?
24. Which atom has a greater nuclear charge, boron or selenium?
Review
PRACTICE:
1. Describe the following:
Alkali metals-
Alkaline earth metals-
Halogens-
Noble gases-
Actinide series
Lanthanide series-
Transition elements-
Main block elements-
2.
Write the periodidc law-
3.
From the periodic table lab, what happened when…
a) Ca and Mg were mixed with HCl
b) CaO and MgO were mixed with H2O
c) CaCl2 and MgCl2 were added to NaCO3
c)
NaCl and NaBr and NaI were mixed with AgNO3
d) K and Na were mixed with water
Fill In the Following chart:
Ionization
energy
Down group
Electronegativity
.
Electron
affinity
Atomic radius
Across period
define
Which element has the largest atomic radius- Zr, In, Nb, I, Sr?
Which element has the smallest ionization energy? O, S, Se, Te, Po
Which element has the smallest electronegativity? Li, F, Be, N, C, O
How did Mendeleev arrange the periodic table?
How did Mosely?
Sheilding
effect