Transcript 2 periodic table cp

Day 4 2-18
1. Which metal would you expect to
be more reactive - Fr OR Cu?
WHY?
2. Which nonmetal would you
expect to be more reactive - F
OR Ne? WHY?
How is the periodic
table arranged?
Periodic Trends
Atomic radius:
- Measure of size – radius of an
atom
- Atoms with more electrons do
NOT necessarily have a larger
atomic radius
Periodic Trends
- Atoms with more electrons do NOT
necessarily have a larger atomic
radius
Periodic Trends
- Atoms with more
1. Atoms get larger
electrons do NOT
going down a
necessarily have a
group.
larger atomic radius
2. Atoms get
smaller going
across a period
So why?...
Periodic Trends
- Atoms with more
As you move down
electrons do NOT
a group you
necessarily have a
larger atomic radius increase the
number of energy
levels in the atom
and so the atom
gets larger as
expected.
Periodic Trends
- Atoms with more As you move across
a period, # of
electrons do NOT
protons increases
necessarily have a
larger atomic radius and outermost
energy level stays
the same, the
attractive force
between elecs. and
pros. pulls the atom
tighter (closer to
nucleus)
Periodic Trends
What’s bigger:
B or Al
B or N
N or Zn
C or Cl
Review
1. What element is in Group 2,
Period 3?
2. Name an element in Group 3
3. How many valence electrons
in Xe?
4. Give me an element with 1
valence electron.
Alkali metalsHalogens
7 valence
1 valence
Nonmetals Noble gases
Magnesium Atomic radius
Ductile
Period 3
metalloids Halogens
inert
1 valence
fluorine
Noble gases
malleable
Atomic radius
Helium
Period 3
Day 5 2-19
1. Why does the size of an atom
decrease moving across a
period?
2. What is more reactive Cl or Ar –
Explain!!!
Review
1. What element is in Group 2,
Period 3?
2. Name an element in Group 3
3. How many valence electrons
in Xe?
4. Give me an element with 1
valence electron.
Partner Review
1. What element is in Group 17,
Period 3?
2. What family of elements is the
element above in?
3. How many valence electrons
does it have?
Periodic Trends
What are ions?
Notes
page 4
- atoms that are charged due
to the loss or gain of
electrons
- If an atom loses elecs. it becomes
smaller and positive
- If an atom gains elecs. it becomes
larger and negative
Periodic Trends
What are ions?
- If an atom loses elecs. it becomes
smaller
- If an atom gains elecs. it becomes
larger
PAGE 176-179
Which elements gain elecs.? Which
elements lose elecs.? Pattern?
Periodic Trends
Elements on the right side of
the periodic table form
negative ions
_________
Elements in the same group
The same ions
form ___________
Periodic Trends
What’s bigger:
F or
F
Na or
+
Na
Na or Rb
Na of Al
F or Cl-
Read / review
Section 6.2 and
complete #s 11-17
on page 173
Day 6 2-22
1. Which halogen is found in period 2?
2. How many valence electrons does
calcium have?
3. Why does the size of an atom
increase moving down a group?
Octet rule – Atoms tend to gain,
lose, or share electrons in order to
acquire a full set of valence
electrons (8)
- 2 for H, He, Li, Be, + B
notes page 6
As of today, you should have the
following:
Families colored in (page 168)
Valence electrons marked
+1, +2, -1,-2, and -3 ions marked
Day 2 3-2
Ions =
Valence
electrons =
+1
1
8
+2
2
3
-3 -2 -1
4 5 6 7
Add today:
Reactivity trend (front / back)
Atomic size (front / back)
Positive and negative ion trend on back
Day 2 3-2
Ions =
Valence
electrons =
Atom size decreases
+1
1
8
Atom size increases
+2
2
3
Reactivity increases away
from the middle
-3 -2 -1
4 5 6 7
Positive and Negative ion trend
Elements on the right side form
negative ions.
Elements on the left form positive
ions.
Read / review Section
6.2 and complete #s
11-17 on page 173
DUE TUESDAY 2-23