Periodic Trends
Increases
What do the dots represent in a Lewis Dot Structure (LDS)?
An Ionic Bond involves a/an _______________ stealing Valence Electrons from a/an ______________.
A). Metal; Nonmetal
B). Nonmetal; Metal
B). Nonmetal; Metal
True or False? It is possible to have a negative Electronegativity Difference value.
b). Where are the Valence Electrons in a NPCoB?
a). A Nonpolar Covalent Bond is where 2 Nonmetals with very similar Electronegativity values equally share Valence Electrons.
b). The Ve- lye in the middle of both Nonmetals with very similar EN values.
Ionization Energy _____________________ when moving across a Period.
Increases
When drawing a Lewis Dot Structure (LDS), where do you start drawing dots?
In the top right corner of the Chemical Symbol for the Element.
Anions ___________ Valence Electrons and have a ____________ charge.
A). lose; positive
B). lose; negative
C). gain; positive
D). gain; negative
D). gain; negative
Atoms with a high Electronegativity value are ______________ that are ______________ at attracting Valence Electrons.
A). Metals; good
B). Nonmetals; bad
C). Metals; bad
D). Nonmetals; good
D). Nonmetals; good
a). Describe a Polar Covalent Bond (PCoB).
b). Where do the Valence Electrons lye in a PCoB?
a). A Polar Covalent Bond is where 2 Nonmetals unequally share Valence Electrons.
b). The Nonmetal with the higher EN value has the Ve- pulled closer to it.
Why does Ionization Energy decrease when moving down a Group?
Because the Atomic Radius increases, which makes it easier to remove Valence Electrons.
When drawing an Lewis Dot Structure for an Element, you can only draw _________ dot(s) on each side first, but later can draw up to ___________ dots on each side.
1; 2
An Ionic Bond involves one Atom _______________ Valence Electrons from the other Atom.
stealing or taking
Atoms with a low Electronegativity value are ______________ that are ______________ at attracting Valence Electrons.
A). Metals; good
B). Nonmetals; bad
C). Metals; bad
D). Nonmetals; good
C). Metals; bad
Draw the Lewis Dot Structure of an H2O Molecule:
a). First with the Covalent Bonds as loops.
b). Then with the Covalent Bonds as lines.
For correct answer, see Covalent Bonds Cornell Notes Part #2, Question #7, Steps #3 and #4.
Cations ___________ Valence Electrons and have a ____________ charge.
A). lose; positive
B). lose; negative
C). gain; positive
D). gain; negative
A). lose; positive
For the Chemical Bond: K---O,
a). Calculate the EN Difference.
b). Determine the Chemical Bond type. (Ionic Bond, Polar Covalent Bond, or Nonpolar Covalent Bond.)
a). 3.5 - 0.8 = 2.7
b). Ionic Bond
Draw the Lewis Dot Structure (LDS) of SiS2 twice.
a). LDS w/ Covalent Bonds (CoB) as loops.
b). LDS w. CoB as lines and lone pairs cleaned up.
For correct answer, see Covalent Bonding Cornell Notes Part #2, Covalent Bonding Quest, #7 CO2. (Your answer should be identical to the last 2 columns here, but with Si instead of C and S instead of O.)
Why does Atomic Radius decrease when moving across a Period?
B/c the number of Protons and Electrons are increasing in the Atom, resulting in an increased Zeff, or Effective Nuclear Charge. This pulls the Electrons closer to the Protons in the Atom, decreasing the Atomic Radius.
When drawing the Lewis Dot Structure (LDS) for an Element, why can you only draw a certain number of dots on each side at one time?
B/c the dots represent Valence Electrons and if you get similar charges too close together, they will repel (bounce off each other), resulting in Energy loss for the Atom.
For the Chemical Bond: Mn---Sb
a). Calculate the EN Difference.
b). Determine the Chemical Bond Type (Ionic Bond, Polar Covalent Bond, or Nonpolar Covalent Bond.)
a). 1.9 - 1.5 = 0.4
b). Nonpolar Covalent Bond
Draw the Lewis Dot Structure (LDS) of AsI3 twice:
a). LDS w/ Covalent Bonds (CoB) as loops.
b). LDS w. CoB as lines and lone pairs cleaned up.
For correct answer, see Covalent Bonding Cornell Notes Part #2, Covalent Bonding Quest, #6 PCl3. (Your answer should be identical to the last 2 columns here, but with As instead of P and I instead of Cl.)
*Don't forget, your Lone Pairs on each I must be angled toward the direction of the Bonding Pair.