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Chemistry-G
Test Review – Chapter 6
Across
1. (two words) is the energy change associated with
the addition of an electron to a gaseous atom
2. type of metals found in the d block of the
periodic table
4. group of elements on the periodic table that are
inert( nonreactive) because they have a low energy
electron configuration
5. (two words) type of metals found in the f block
of the periodic table
7. (two words) is the energy needed to remove the
outermost electron from a gaseous atom
11. a vertical column on the periodic table
12. the tendency of an element to gain electrons
when combining with another element
17. elements found on the left side of the periodic
table that have few outer electrons and tend to form
positive ions by losing electrons
21. last name of person who determined the atomic
masses of many of the elements
Name:
Date:
22. group of elements on the periodic table that
have an outer electron configuration of s1 and form
1+ ions when stable
23. group of elements on the periodic table that
have an outer electron configuration of s2p4 and
form 2- ions when stable
24. group of elements on the periodic table that
have an outer electron configuration of s2p3 and
form 3- ions when stable
Down
1. the most important factor determining the
periodic patterns in the periodic table
3. last name of the first person to try to arrange the
known elements into a table based on increasing
atomic mass
6. group of elements on the periodic table that have
an outer electron configuration of s2p2 and can form
4+ or 4- ions when stable
8. subatomic particle that plays the most important
role in determining the properties of an element
9. states that when you arrange the elements in
order of increasing atomic number you will see a
periodic pattern in the chemical and physical
16. group of elements on the periodic table that have
properties of the elements
an outer electron configuration of s2p5 and form 110. elements that have properties in between metals
ions when stable
and nonmetals
18. is the effect that inner energy levels have by
13. (two words) group of elements on the periodic table
blocking out the nuclear charge
that have an outer electron configuration of s2 and form
19. group of elements on the periodic table that have
2+ ions when stable
an outer electron configuration of s2p1 and form 3+
14. elements found on the right side of the periodic
ions when stable
table that have many outer electrons and tend to form
20. a horizontal row on the periodic table
negative ions by gaining electrons
15. (two words) is the effect that the number of protons
in the nucleus has on the outer electrons
B. Matching:
_____21. energy associated with the addition of an electron to a gaseous atom a. electronegativity
_____22. tendency of an element to gain electrons when combining
b. electron affinity
with another element
c. ionization energy
_____23. energy needed to remove an electron from a gaseous atom
d. all of the above (a, b and c)
_____24. increases across a period due to nuclear charge
e. atomic size
_____25. decreases across a period due to nuclear charge
_____26. increases down a group due to shielding
_____27. decreases down a group due to shielding
C. Answer true or false:
_____28. The noble gases have an unstable electron configuration.
_____29. The noble gases are inert ( chemically unreactive).
_____30. The alkali metals are never found in the uncombined state in nature.
_____31. The alkaline earth elements have an outer electron configuration of s1.
_____32. The alkali metals have an outer electron configuration of s2.
_____33. The halogens have outer electrons with an s2p5 electron configuration.
_____34. Most of the noble gases have outer electrons with an s2p6 electron configuration.
_____35. The halogens have a very stable electron configuration.
_____36. Group 1A contains the halogens.
_____37. Group 7A contains the alkali metals.
_____38. Group 0 contains the noble gases
_____39. Group 2A contains the alkaline earth elements
_____ 40. Metals lack luster and are poor conductors of electricity.
_____ 41. Nonmetals have many electrons in their outer energy levels and tend to gain electrons to become
stable.
_____ 42. Nonmetals tend to form negative ions by gaining electrons.
_____ 43. Silicon is a semiconductor.
_____ 44. The Mg2+ ion is bigger than the Mg atom.
_____ 45. The Na+ ion is larger than the Mg2+ ion.
_____ 46. The nitride ion (N3-) is larger than the oxide (O2-) ion.
_____ 47. The barium(at. No. 56) atom is smaller than the strontium atom(at. No. 38).
_____ 48. Calcium has a higher electronegativity than magnesium.
_____ 49. Sodium has a higher electron affinity than magnesium.
_____ 50. Fluorine has a very high electronegativity.
_____ 51. The representative elements are found in the d and f blocks of the periodic table.
_____52. The alkali metals form hydroxides (bases) when added to water.