Transcript 4 periodic table cp

Q of the Day
Day 6 3-10
1. The octet rule explains that
8 valence
Sulfur wants ___
2 and
electrons so it will gain ___
form a ____
-2 ion.
Periodic Trends
Ionization energy – energy
needed to remove one electron
from an atom
Li → Li+ + eionization energy = 8.64e-19 J/atom
… indication of how strongly an atom
holds onto its outermost elecs.
Periodic Trends
First ionization energy (kJ/mol)
The graph on page 178 shows how
ionization energies vary with atomic #
Atomic number
Periodic Trends
First ionization energy (kJ/mol)
What element does the
point at (5, 800) represent?
Atomic number
Periodic Trends
With respect to the periodic
table ionization energies show 2
important trends…
1. Decrease as you move down
a group
2. Increase as you move left to
right across a period
Periodic Trends
How does the ionization energy
trend compare to the atomic
radius trend?
Does this make sense?
Periodic Trends
What’s bigger:
O or C
↑er I. E.:
O
Be or Ca
Be
Na or Be
Be
Cl of Al
Cl
Ca or
+3
B
-----
Read Section 6.3
and complete #s
18-25 on page 182
Day 1 3-11
1. Which of the following are larger?
Ne OR Br-1  Give all 3 reasons why
(BE SPECIFIC!).
2. Why are Ar and Kr both in group
18??
3. Why are H and He both in
period 1?
Day 2 3-12
1. Get out your lab, which unknowns
turned pink with the addition of
solution C (when you are done you
should have 3)?
Day 3 3-13
Hints for your lab data:
- every solution should form one
precipitate (either with A or B)
- 3 of your solutions should turn
pink with the addition of C
- 6 of your precipitates should
dissolve with the addition of D
Day 4 3-16
1. Get out your lab, postlab, and
review!!!
2. The test will be Friday 3-20.
3. Postlabs (both parts) are due
Wednesday 3-18.
4. The review should be finished by
Thursday 3-19.
Day 5 3-17
1. What are 3 things that ALL noble
gases have in common?
Periodic Trends
Successive Ionization energies
(removing more than one
electron from an atom):
- The 2nd > 1st, the 3rd > 2nd,
the 4th > the 3rd
- but if you look think about I. E. s there
is usually a large jump. Where?
As of today, you should already have the
following:
Families colored in (page 168)
Valence electrons marked
+1, +2, -1,-2, and -3 ions marked
Reactivity trend (front / back)
Atomic size (front / back)
Electronegativity (front / back)
Added today:
Ionization energy (front / back)
Ionization energies are higher for
smaller atoms!
Day 5 3-17
Day 5 3-17
1. Get out your lab, postlab, and review!!
2. The test will be Friday 3-20 and you
will hand in your colored periodic
table.
3. Postlabs (both parts) are due
tomorrow.
4. The review should be finished by
Thursday 3-19.
YOU WILL HAVE EXACTLY 3
MINUTES FROM THE TIME
THE BELL RINGS TO FINISH
AND THEN HAND IN YOUR
ATB.
Day 6 3-18
1. Which of the following are larger?
Na OR Be+2  Give at least 2 specific
reasons why.
2. Why are Mg and Sr both in group 2?
3. Why are the alkali metals and the
halogens so reactive?
Day 6 3-18
1. Which of the following are larger?
Al+3 OR Rb  Give at least 2 specific
reasons why.
2. Why are Mg and S both in period 3?
3. Why are the alkali metals and the
halogens so reactive?
Day 6 3-18
1. Which of the following are larger?
Cl- OR Ne  Give at least 2 specific
reasons why.
2. Why are Br and I both in group 17?
3. Why are the alkali metals and the
halogens so reactive?
Day 6 3-18
1. Which of the following are larger?
Ar OR Se-2  Give at least 2 specific
reasons why.
2. Why are Na and S both in period 3?
3. Why are the alkali metals and the
halogens so reactive?
Day 6 3-18
1. Get out your lab, postlab, and
NOTES!!!
2. The test will be Friday 3-20 and you
will hand in your colored periodic
table.
3. Postlabs (both parts) are due NOW.
4. The review should be finished by
Thursday 3-19.
How does atomic radius change?
Bigger down a group and smaller
across a period
Why?
As you move down a group, there are
additional energy levels
As you move across a period there are
additional protons pulling the electron
in tighter
How does ion size change?
Negative ions get bigger
Positive ions get smaller
Why?
Negative ions gain electrons
Positive ions lose electrons
How does ionization energy
change?
Opposite of size (atomic radius)
Why?
Electrons are closer to the nucleus
and held tighter in smaller atoms
How does reactivity change?
Away from the middle
Why?
Atoms on the outside of the p.t.
are closer to achieving the octet
rule and so more reactive
How does electronegativity
change?
Increases up and to the right (Fr to
F)
Why?
Elements on the right side of the
periodic table want electrons to
satisfy the octet rule
YOU WILL HAVE EXACTLY 3
MINUTES FROM THE TIME
THE BELL RINGS TO FINISH
AND THEN HAND IN YOUR
ATB.
Day 1 3-19
1. Which of the following are larger?
Ne OR Br-1  Give 2 reasons why (BE
SPECIFIC!).
2. Why are Ar and Kr both in group 18??
3. Why are H and He both in
period 1?
Day 1 3-19
1. Which of the following are larger? F-1 OR He
 Give 2 reasons why (BE SPECIFIC!).
2. Why are Cs and Ba both in period 6??
3. Why are H and K both in
group 1?
Day 1 3-19
1. Which of the following are larger?
Sr+2 OR Cs  Give 2 reasons why (BE
SPECIFIC!).
2. Why are Br and I both in group 17??
3. Why are Be and N both in
period 2?
Day 1 3-19
1. Which of the following are larger?
B+3 OR Mg  Give 2 reasons why (BE
SPECIFIC!).
2. Why are Kr and Ne both in group 18??
3. Why are Al and Cl both in
period 3?
Day 1 3-19
1. Get out your REVIEW!!!
2. The test will be Friday 3-20 and you
will hand in your colored periodic
table.
3. Postlabs (both parts) are late.
4. The review should be finished by
NOW.
The test will be FRIDAY 3-20!!!
BRING your COLORED PERIODIC
TABLE and your REVIEW!!!