Name __________________________
Period _________
Exploring Bonds: Intro Activity
You will be answering these questions as a group WITHOUT the help of your
teacher. Remember that time ticks, and you must be on task without side
conversations!
1) Define covalent bond. How is a covalent bond like peanut butter between two slices
of bread? (2 sentences)
2) Define ionic bond. How is a covalent bond different from an ionic bond?
3) Unlike Bohr Diagram, Lewis dot structures show the element and the valence
electrons found in that element. You put one electron on each side and then you start
pairing the electrons. Some examples are shown below. Complete the Lewis dot
structures for the remaining elements.
C
O
Be
K
Cl
Al
Ge
Te
Ar
F
N
B
4) A pair of electrons that are not being shared, in other words, they are not bonded to another atom are called
lone pairs (They are lonely pairs of electrons). Indicate which electrons are shared as bonds (bonding) and
which electrons are the nonbonding lone pairs in drawing B. There is an example for you in drawing A.
Bonding
electrons
Lone pairs
Lone pair
4c) Do you think each element in the compounds above satisfy the octet rule? Explain
your observation as a group. Normally how many valence electrons does hydrogen have
and how many does fluorine have? What happens after H and F bond?
5. You must know a few things about molecular structures. Hydrogen can hold two
electrons max, it will NEVER have a double nor triple bond. Each line represents a bond.
Instead of writing two electrons in the form of dots, we chemists write a line instead.
When you see a line, see it as two imaginary electrons. Label the following on the
following two structures: 1) Lone pairs 2) single bonds 3) double bonds 4) triple
bonds. Note: all elements satisfy the octet rule, do you see that? Discuss this in your
group.
6. Play with the puzzle pieces, what factor determines how many dots are on each
puzzle piece?
7) Once you fit the pieces together (creating a covalent bond), is the octet rule
satisfied?
DRAW one example below (using puzzle pieces) and explain your reasoning. What does
this tell you about how elements bond?
8) Using the given molecular formula (HF for example), draw what each molecule looks
like by replacing teach pair of shared electrons with a line (bond – representing 2
electrons). An example is clearly shown below:
NH3
H3CCH3
CH2ClBr
H2S
CH4
H20
PH3
N2H4
9) How many bonds does carbon (C) typically form?
10) Does your answer to #9 make sense based on the number of valence electrons that C
needs to share to obtain a full valence shell? Explain.
11) How many bonds does N typically form?
12) Does the answer to question #11 make sense based on the number of valence
electrons that N needs to share to obtain a full valence shell? Explain.
13) How many bonds does O typically form?
14) Does the answer to question #13 make sense based on the number of valence
electrons that O needs to share to obtain a full valence shell? Explain.
15) How many bonds do H, F, Cl, and Br typically form?
16) Does the answer to question 15 make sense based on the number of valence
electrons that H, F, Cl, and Br need to share to obtain full valence shells? Explain.
17) Based on question 15, explain why you think H, F, Cl and Br are most likely to be
end (terminal) atoms rather than central (bridging) atoms in a molecule. Think about it
as a group. Really, really, think!