Transcript Test Review

Unit 3
Marker Board Review
Make sure you have the following ready
•Marker board and marker
•Periodic table
1. ________________
Dmitri Mendeleev created the first
periodic table which was arranged
according to atomic _____.
mass
2. In the modern periodic table, elements are
ordered by atomic ________.
number
______________
Henry Moseley was the first scientist to
order them this way.
3.
__________ law says that when the elements
Periodic
are placed in order by atomic number there is a
periodic repetition of their chemical and physical
properties.
4. Number
____________________
of protons determine the identity
of an element and the atomic number.
5.
2, 13-18
Groups1,___________________
are
known as the representative elements
because…
They act…..
6.
The valence electrons of representative
p orbitals.
elements are in the __
s and __
Metals
7. Group 1: called the _______
They have
Alkali metals.
1
s
electron configurations ending in __. Properties of these
elements include:
Extremely reactive, soft in nature
a. Stored in ___
oil due to extreme reactivity with oxygen
(contains the most reactive metal)
butter
b. Consistency is ________.
electricity
heat and ___________.
c. Good conductors of ____
8. Group 2: called the _____________
Alkaline-Earth metals.
Their electron configurations end in __.
s2
Properties of these elements include:
Here are some props
soft solids.
a. generally ____
b. _______
Harder and denser than alkali metals
reactive than alkali metals.
c. Less _______
9. Thetransition
___________ metals are a large group of elements in the
middle of the periodic table. Properties of these elements include:
a. Transition metals are also known as the __-block
elements
d
b. General properties (similar to other metals) are…
Properties…
c.Most transition metals are hard
_____ solids with high
_____ melting points.
d.Transition metal unpaired d-electrons have the ability to move into
the s
__ level. Because of this, many transition metals can form
several different charged ions.
e. Transition metals contain the __________
preciousmetals (like gold &
silver)
10. The inner
______________
transition metals are also
known as the f-block. The elements in this
radioactive
block are very ____________.
Nonmetals
11. Group 17 is thehalogen
_________ family. Their electron configurations
2p5 Properties of these elements include:
end in s_____.
properties
a. Veryreactive
_________ nonmetals – they are always in compounds, never
alone.
b. Halogens tend to gain or share 1 electron because they have7__
valence electrons.
d. The most reactive nonmetal, fluorine
_________, is in this family.
e. Exist in all 3 _______
states of matter (s, l, g)
metals especially alkali, to produce salts.
f. React readily with ________,
(halogen = salt former)
12. Group 18 elements are the _______
noble gases. Their
electron configurations end in _____.
s2p6 Properties of
these elements include: Nonreactive, gases,
a. Called inert or ______
noble gases because….
Their outermost energy level is full meaning
they don’t need more electrons from other
elements.
14. The reason any group has similar properties is because
Valence electrons
they have the same number of _________________
Hydrogen
only element considered to be a chemical family all by itself.
15. Hydrogen is placed in group 1 because it has __
1 valence
electron.
16. Hydrogen has properties of group 1 and group
17
________.
Match the family name to the location:
C lanthanides and actinides (inner transition metals)
20. ___
A alkali and alkaline earth metals
21. ___
22. ___
D halogens
23. ___
E noble gases
24. ___
B transition metals
p
25. Label the s, p, d and f
blocks on the periodic
table.
s
d
f
26. An element has the electron configuration
[Ne]3s23p5.
What family is this element in? halogen
_________
What group? 17
____________
What period? __
3
What is this element? Chlorine
__________________
Match the element with the family to which it belongs:
27. neon
______
E
28. magnesium
______
B
a = alkali metals
29. fluorine
______
D
b = alkaline earth metals
30. silver
______
C
c = transition metals
31. potassium
______
A
d = halogens
32. iron
______
C
e = noble gases
Use the following words to fill in the blanks.
A = alkali metals
B = alkaline-earth metals C = transition metals
D = halogens
E = noble gases
B
33. The ____ have electron configurations that end in s2.
A
34. The ____ are soft enough to cut with a knife.
C
35. The ____ contain the precious metals.
D
36. The ____ are the most reactive nonmetals.
E
37. The ____ are stable and unreactive due to their full s and p orbitals.
D
38. The ____ have a name that means salt-former.
Periodic Trends
39. As you move down a group on the periodic table,
atomic radii generally _______________
gets larger and across a
period it generally __________________.
gets smaller
Periodic Trends
40. Define ionization energy.
Energy needed to remove an electron from an atom
41. Ionization energy generally _____________
gets larger across a period and
______________
gets smaller down a group.
42. Which family of elements has the highest ionization energy?
______________
Noble gases
43. The tendency for an atom to attract electrons of another atom is
increases as you
electronegativity It generally ___________
called __________________.
move left to right across a period and __________
decreases down a group.
Circle the atom with the LARGER atomic radius
44.
cesium
potassium
45.
sodium
aluminum
46.
cesium
helium
Circle the atom with the LARGER ionization energy
47. boron
48. nitrogen
49. chlorine
oxygen.
phosphorous
selenium
Circle the atom with the LARGER electronegativity
50. calcium
potassium
51. fluorine
bromine
52. phosphorus
oxygen
53. Be prepared to describe how the trends change across or
down the periodic table.