day 4 3-6 1.which of the following are larger? f or s -2 2. give all 3 reasons why (be specific!)
DESCRIPTION
1.Which of the following are larger? Ca OR Sr Cs OR Cs +1 Rb OR Ca +2TRANSCRIPT
Day 4 3-61.Which of the following are
larger?
F OR S-2
2. Give all 3 reasons why (BE SPECIFIC!).
How is the periodic table arranged?
1. Which of the following are larger?
Ca OR Sr
Cs OR Cs+1
Rb OR Ca+2
Partner Review1. 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?
4. Which is more reactive Ne or F?
Day 5 3-91. Why are Na and K both in
group 1?
2. Why are Na and Mg both in period 3?
How is the periodic table arranged?
Electronegativity – ability to attract electrons in a bond
Na—Cl
… In the compound above electrons shift toward Cl because it is more electronegative!
Notes page 6
What is electronegativity?
How does it increase on the p. t. ?
Electronegativity – ability to attract electrons in a bond
How does it increase on the p. t. ?
In this bond: Mg—O, which way do elecs. Shift? WHY?
O, > electroneg.
Metals
Halogens
Octet rule
Ion
Alkali metals
Noble gases
electronegativity
Alkaline metals
Atomic size
Period 2
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)
Added today:
Electronegativity (front / back)
Day 5 3-9
Valence electrons =
2
1
3 4 5 6 7
8
Ions = +1
+2 -3 -2 -1
Atom size decreases
Atom
size increases
Reactivity increases away from the middle
Electronegativity
increases from Fr to F
Read Section 6.3 and complete #s
18-25 on page 182