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A Chemical Bond Between Atoms Results From The Attraction Between The Valence Electrons And ______
Of Different Atoms.
Nuclei
A Covalent Bond Consists Of ....
A Shared Electron Pair
What Is A Polar Covalent Bond?
a Covalent Bond In Which The Electrons Are Not Shared Equally Between The Atoms, Resulting In A Partial Positive And Partial Negative Charge.
The Electrons Involved In The Formation Of A Chemical Bond Are Called
Valence Electrons
What Is A Molecule?
A Molecule Is A Neutral Group Of Atoms That Are Held Together By Covalent Bonds.
FILL IN THE BLANK
The Two Nuclei & Two Electrons ..... Each Other
Repel
FILL IN THE BLANK
The Electron Of One Atom & Proton Of The Other Atom ..... One Another.
Attract
A Chemical Compound Whose Simplest Units Are Molecules Is Called A....
Molecular Compound
Atoms With A Strong Attraction For Electrons They Share With Another Atom Exhibit....
High Electronegativity
A Bond's Character Is More Than 50% Ionic If The Electronegativity Difference Between The Two Atoms Is Greater Than .....
1.7
How Do You Determine The Molecular Shape Of A Covalent Compound?
It Is Determined By The Arrangement Of Its Atoms And The Number Of Electron Pairs Around The Central Atom.
What Is A Molecular Formula?
It Shows The Types & Number Of Atoms Combined In A Single Molecule Of A Molecular Compound
Bond Energy
The Greater The Electronegativity Difference Between Two Atoms Bonded Together, The Greater The Bond's percentage Of....
Ionic Character
What are Lewis structures?
Lewis structures are diagrams that represent the arrangement of atoms and valence electrons in a covalent compound.
Using the following electronegativity values, classify the bonding between carbon, C, and the following elements: hydrogen, H; oxygen, O; and nitrogen, N. In each pair, which atom will be more negative?
The electronegativity of carbon is 2.5. The electronegativities of hydrogen, oxygen, and nitrogen are 2.1, 3.5, and 3.0
1)2.5-2.1= 0.4 Polar
2)3.5-2.5= 1 Polar
3)3.0-2.5= 0.5 Polar
Using the following electronegativity values, classify the bonding between sodium, Na, and the following elements: chlorine, Cl; oxygen, O; and sulfur, S. In each pair, which atom will be more negative?
The electronegativity of sodium is 0.93. The electronegativities of chlorine, oxygen, and sulfur are 3.0, 3.5, and 2.5.
1)3.0-0.93= 2.07 Ionic
2)3.5-0.93= 2.57 Ionic
3)2.5-0.93= 1.57 Polar
Using the following electronegativity values, classify the bonding between nitrogen, N, and the following elements: hydrogen, H; fluorine, F; and phosphorus, P. In each pair, which atom will be more negative?
The electronegativity of nitrogen is 3.0. The electronegativities of hydrogen, fluorine, and phosphorus are 2.1, 3.98, and 2.19.
1)3.0-2.1=0.9 Polar
2)3.98-3.0=0.98 Polar
3)3.0-2.19=0.81 Polar
Using the following electronegativity values, classify the bonding between aluminum, Al, and the following elements: oxygen, O; chlorine, Cl; and silicon, Si. In each pair, which atom will be more negative?
The electronegativity of aluminum is 1.61. The electronegativities of oxygen, chlorine, and silicon are 3.5, 3.0, and 1.9.
1)3.5-1.61=1.89 Ionic
2)3.0-1.61=1.39 Polar
3)1.9-1.61=0.29 Non Polar
Using the following electronegativity values, classify the bonding between oxygen, O, and the following elements: lithium, Li; nitrogen, N; and fluorine, F. In each pair, which atom will be more negative?
The electronegativity of oxygen is 3.5. The electronegativities of lithium, nitrogen, and fluorine are 0.98, 3.04, and 3.98.
1)3.5-0.98=2.52 Ionic
2)3.5-3.04=0.46 Polar
3)3.98-3.5=0.48 Polar
Draw Lewis Structures to represent each of the following formulas:
NH3
..
H-----N------H
l
H
Draw Lewis Structures to represent each of the following formulas:
H2O
..
H----O----H
..
Draw Lewis Structures to represent each of the following formulas:
CH4
H
l
H------C-----H
l
H
Draw Lewis Structures to represent each of the following formulas:
C2H2
----
H-----C-----C----H
----
Draw Lewis Structures to represent each of the following formulas:
CH2O
:O:
l
l
C
/ \
H H