Transcript Unit 3 Review - RHSChemistry

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. However,
_________
electrons determine the chemical behavior.
5.
1, 2, 13-18 (or 1A-8A) are
Groups ___________________
known as the representative elements.
6.
The valence electrons of representative
p orbitals.
elements are in the __
s and __
Metals
7. Group 1: called the _______
Alkali metals. They have
1 Properties of these
electron configurations ending in s__.
elements include:
Extremely reactive, soft in nature
a. Stored in ___
oil due to extreme reactivity with oxygen
(contains the most reactive metal)
b. Form ____
+1 (charge) ions. Metals are positive losers
c. Good conductors of ____
electricity
heat and ___________.
8. Group 2: called the _____________
Alkaline-Earth metals.
Their electron configurations end in __.
s2
Properties of these elements include:
soft solids.
a. generally ____
b. _______
Harder and denser than alkali metals
c. Less reactive
_______ than alkali metals. Yet more
reactive than
+2 (charge) ions.
d. Form ___
the transition
metals
transitionmetals are a large group of elements in the
9. The ___________
middle of the periodic table. Properties of these elements include:
10. Transition metals are also known as the __-block
elements
d
11. General properties (similar to other metals) are…
a.Most transition metals are _____
_____ melting points.
hardsolids with high
b.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.
c. Transition metals contain the __________
precious metals (like gold &
silver)
12. The ______________
inner transition metals are also
known as the f-block. The top row is called
the Lanthanides
___________ and the bottom row the
Actinides This group contains synthetic
________.
and radioactive metals.
Nonmetals
13. Group 17 is thehalogen
_________ family. Their electron configurations
2p5 Properties of these elements include:
end in s_____.
a. Very _________
reactivenonmetals – they are always in compounds, never
alone.
b. Halogens tend to gain or share 1 electron because they have __
7
valence electrons.
c. Form ___
-1 (charge) ions. Nonmetals are negative gainers
d. The most reactive nonmetal, _________,
fluorine is in this family.
e. Exist in all 3 _______
states of matter (s, l, g)
f. React readily with ________,
metals especially alkali, to produce salts.
(halogen = salt former)
14. Group 18 elements are the _______
noble gases. Their
electron configurations end in _____.
s2p6 Properties of
these elements include:
a. Called inert or ______
noble gases because….
Their outermost energy level is full meaning
they don’t need more electrons from other
elements.
b. Do not form _____
ions or ______.
bonds
15. The reason any group has similar properties is because
they have the same number of _________________
Valence electrons
Hydrogen
only element considered to be a chemical family all by itself.
16. Hydrogen is placed in group 1 because it has __
1 valence
electron.
17. Hydrogen has properties of group 1 and group
________.
1 & 17
18. The universe is __________%
hydrogen by mass.
90
Match the family name to the location:
C lanthanides and actinides (inner transition metals)
19. ___
A alkali and alkaline earth metals
20. ___
21. ___
D halogens
22. ___
E noble gases
23. ___
B transition metals
p
24. Label the s, p, d and f
blocks on the periodic
table.
s
d
f
25. An element has the electron configuration
[Ne]3s23p5.
What family is this element in? halogen
_________
What group? 17
____________
or (7A)
What period? __
3
What is this element? Chlorine
__________________
Match the element with the family to which it belongs:
26. neon
______
E
27. magnesium
______
B
a = alkali metals
28. fluorine
______
D
b = alkaline earth metals
29. silver
______
C
c = transition metals
30. potassium
______
A
d = halogens
31. 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
32. The ____ have electron configurations that end in s2.
A
33. The ____ are soft enough to cut with a knife.
C
34. The ____ contain the precious metals.
D
35. The ____ are the most reactive nonmetals.
E
36. The ____ are stable and unreactive due to their full s and p orbitals.
D
37. The ____ have a name that means salt-former.
Periodic Trends
38. As you move down a group on the periodic table,
atomic radii generally _______________
gets larger and across a
period it generally __________________.
gets smaller
• Gets larger because as you move
down a group, an energy level is
added, which blocks the power
of the nucleus to pull in.
• gets smaller because the more
protons an atom has the stronger
the pull of the nucleus and the
smaller the atom becomes.
Periodic Trends
39. Define ionization energy.
Energy needed to remove an electron from an atom
40. Ionization energy generally _____________
gets larger across a period and
______________
gets smaller down a group. • gets larger because the
atomic radius is getting
• gets smaller because the atomic
smaller, which makes it
radius is getting larger, which
more difficult to take an
makes it easier to remove an
electron
electron
41. Which family of elements has the highest ionization energy?
______________
Noble gases
42. The tendency for an atom to attract electrons of
electronegativity
another atom is called __________________.
It
increases
generally ___________
as you move left to right
decreases
across a period and __________
down a group.
•
Increases because as the
ionization energy goes up
and the atomic radius goes
down, the atom will hold
onto electrons shared in a
bond more. If an atom will
hold onto its own electrons
tightly, it will hold onto
shared electrons tightly.
•
Decreases because as the ionization
energy goes down and the atomic
radius goes up, the atom won’t hold
onto electrons shared in a bond as
tightly. If an atom won’t hold onto
its own electrons tightly, it won’t
hold onto shared electrons tightly.
This group of elements doesn’t have an
electronegativity _______________________
Noble gases, because they don’t form
compounds
Be prepared to justify your answers.
Circle the atom with the LARGER atomic radius
43.
cesium
potassium
44.
sodium
aluminum
45.
cesium
helium
Circle the atom with the LARGER ionization energy
46. boron
47. nitrogen
48. chlorine
oxygen.
phosphorous
selenium
Circle the atom with the LARGER electronegativity
49. calcium
potassium
50. fluorine
bromine
51. phosphorus
oxygen
Be prepared to justify your answers.