Unit 3 Review!
Section 6.1

Dmitri Mendeleev
_________________created
the first
periodic table which was arranged
according to atomic ___________.
Mass
Pudding
1.
In the modern periodic table, elements
Number
are ordered by atomic __________.
Henry Moseley
______________
was the first scientist
to order them this way.
Wedding cake
•
Periodic
______________
law says that when
the elements are placed in order by
atomic number there is a periodic
repetition of their chemical and physical
properties.
HUGE PIZZA!!!!!
1.
_______________
determine the
Protons
identity of an element and the atomic
Electrons
number. However, _______________
determine the chemical behavior.
Chapter 7
1.
Study your notes for metals,
nonmetals, and metalloids. Be sure
you could identify elements of these
regions and describe the properties of
these regions.
1.
1A-8A
Groups _____________________
are
known as the representative elements
because…
They possess
a wide range of
properties

The valence electrons of representative
P
S
elements are in the ____
and ____
orbitals
Group 1 elements

Alkali
Group 1: called the _____________
metals. They have electron
configurations ending in ________.
s1
Properties of Group 1 elements include:
1. Stored

in _________
due to extreme
oil
reactivity with oxygen (contains the
most reactive metal)
1+
2. Form __________
(charge) ions.
3. Consistency is ________.
Cold Butter
Electricity
Heat and _______
Good conductors of _____
Group 2 elements

Group 2: called the
Alkaline
Earth
________metals.
Their electron
configurations end in
s2
______________.
Properties of Group 2 elements
include:

Shiny
generally _____________
solids.
Harder
1. ________and
denser than alkali metals
reactive
2. Less ______________
than alkali metals.
2+
3. Form __________________
(charge) ions.

Transition
The ____________________
metals are a large group of
elements in the middle of the periodic table. Properties
of these elements include:
Properties of Transition metals
include:
2.
Transition metals are also known as the _____-block
d
elements
General properties (similar to other metals) are…
1.
Electrical conductivity, lustrous, malleable
Most transition metals are _______
High
Hard solids with ________
1.
2.
3.
4.
melting points.
Transition metal unpaired d-electrons have the ability to
move into the ________
valence level. Because of this, many
transition metals can form several different charged ions.
precious
Transition metals contain the ________________
metals
(like gold & silver)
The more unpaired electrons in the d-level, the …..
The greater the hardness and the
higher the melting and boiling point
•
Inner Transition
The _______________________
metals are also known as
the f-block. The top row is called the _____________
Lanthanides and the
Actinides
bottom row the ________________.
This group contains
synthetic and radioactive metals.
Group 17

Halogen
Group 17 is the ______________________
family. Their electron configurations end in
_________.
P5
Properties of elements in group 17:

reactive
Very ___________
nonmetals – they are
always in compounds, never alone.
1.
2.
3.
4.
5.
Halogens tend to gain or share 1 electron because
7
they have ________
valence electrons.
1Form ________
(charge) ions.
The most reactive nonmetal,
Fluorine
__________________,
is in this family.
Exist in all 3 ____________
of matter (s, l, g)
States
Metals
React readily with ____________,
especially alkali,
to produce salts. (halogen = salt former)
Group 18 elements

Noble
Group 18 elements are the _______
gases. Their electron configurations
end in _______.
P6
Properties of group 18 elements
include:
1.
Noble
Inert or _________
gases because….
Full outer shell of e-
1.
Do not form ions or bonds.
•
The reason
any group
has similar
properties is
because they
have the
same
number of
Valence e__________.
Hydrogen:




only element considered to be a chemical
family all by itself.
Hydrogen is placed in group 1 because it
has _________
valence electron.
1
Hydrogen has properties of group 1 and
group ___________.
7a
The universe is _____%
hydrogen by
90
mass.

Hydrogen acts like a metal when…..
It loses an electron

Hydrogen acts like a nonmetal when…
It gains an electron
Match the family name to the location:
______
C lanthanides
and actinides
(inner transition
metals)
_______alkali
and
A
alkaline earth
metals
_______halogen
D
_______noble
gases
E
_______transition
B
metals
e
a
d
b
Label the s, p, d and f blocks on the
periodic table above
c
•
An element has the electron configuration
[Ne]3s23p5. What family is this element in?
Halogens
Halogens What period?
_______ What group? ________
____________
What is this element? Chlorine
_______
3
Match the element with the family
to which it belongs:

Neon

Magnesium

Fluorine

Silver



a=Alkaline Metals

b=Alkaline Earth Metals

c=Transition Metals

d=Halogens

e=Noble Gasses
Potassium
Iron
A = alkali metals B = alkaline-earth metals
C = transition metals
D = halogens
E = noble gases
The __________________
have electron configurations that end in s2.
B
The _______________________
are soft enough to cut with a knife.
A
The ______________________
contain the precious metals.
C
The ______________________
are the most reactive nonmetals.
D
The _______________
are stable and unreactive due to their full s and p orbitals.
E
The ___________________
have a name that means salt-former.
D
•
•
As you move down a group on the
periodic table, atomic radii generally
Increases
____________
and across a period it
Decreases
generally _______________.
Review your notes and know why!
•
Define ionization energy.
Energy needed to remove an e- from an atom
What did one ion say to the
other ion?
I got my ion you!
•
•
Increases
Ionization energy generally __________
across a period and ______________
Decreases
down a group.
Review your notes to explain why.
A small furry mammal walks into a bar and orders a drink. The
bartender says, "Sorry, our maximum occupancy is only 6.00 x
1023. We can't serve a mole."
•
Which family of elements has the
highest ionization energy?
Noble Gases
______________
•
•
The tendency for an atom to attract
electrons of another atom is called
______________.
It generally
Electronegativity
____________
as you move left to right
Increases
across a period and _____________
Decreases
down a group.
Know Why! Review your notes.
Circle the atom with the LARGER atomic radius
cesium
 sodium
 cesium

potassium
aluminum
helium
Circle the atom with the LARGER ionization energy
Boron
 nitrogen
 Chlorine

oxygen
phosphorous
selenium
Circle the atom with the
LARGER electronegativity



calcium
fluorine
phosphorus
potassium
bromine
oxygen