Covalent bonding patterns
write the lewis dot structure for the elements below by adding the correct number of dots around each of the element symbols.
a. f b. n c. c d. o
for each element in question 1 replace each unpaired electron (or dot) with a bond (dash) and add an h atom to it.
count the number of electrons around the elements above. remember that each bond (dash) you draw represents two electrons. do each of your elements have eight electrons around them?
using the formula “8 – number of valence electrons” you can predict the number of bonds formed by an element. for each element listed below, determine the number of bonds that each will make. for example: carbon, c : 8 – 4 (valence) = 4 bonds .
5. a. chlorine, cl: b. sulfur, s: c. phosphorous, p: d. silicon, si:
for each of the group 7a elements shown below, construct the correct number of bonds to the element. refer to page 186 in your text for locating group 7a.
6. a.
for each of the elements below, make the correct number of bonds to the element. they are elements in group 6a. refer to page 186 in your text for locating group 6a.
a. f b. cl c. br d. i b. what is the pattern observed? how many bonds does each form?
a. o b. s c. se d. te b. what is the pattern observed? how many bonds does each form?

write the lewis dot structure for each of the elements shown below:
a. na f b. mg o
in an ionic bond, unpaired valence electrons are transferred from the metal to the nonmetal element. in the structures of question 1, label each element as metal or nonmetal then circle each electron dot on the metal and draw an arrow to where the electron will go around the nonmetal to make a pair.
a. na f b. mg o
3. when a metal atom “gives” away one or more electron, the metal becomes positive and the nonmetal gaining the electron(s) becomes negative. place the appropriate charge (+ or –) to the upper right of each of the elements below. na is done for you. if two electrons are transferred, the charge is 2+ or 2-.

4.
a. na f b. mg o
look at the electron configurations for the following metal elements. write down how many electrons each element will lose to become a noble gas. write the element symbol and the charge of the ion formed. 2261 +
5.
in the table below write the electron configuration for each of the ions. identify the noble gas that the configuration represents.
for example: 1s 2s 2p 3s ; # of electrons lost:
1 ; ion formed: na ion formed:
ion formed: ion formed:
1s22s22p63s23p64s2 ;
1s22s22p63s23p1;
1s22s22p63s23p64s1;
# of electrons lost: ; # of electrons lost: ; # of electrons lost: ;
ion
configuration
noble gas
ca2+

s2–

n3–

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