Ionic Compounds 7.4 Metallic Bonds and the Properties of Metals.
Chemistry Matter and Change Chapter 7 Ionic Compounds and Metals.
-
Upload
gwen-warner -
Category
Documents
-
view
237 -
download
0
Transcript of Chemistry Matter and Change Chapter 7 Ionic Compounds and Metals.
Previous
Ca: 1s22s22p63s23p64s2
Ar: 1s22s22p63s23p6
Draw the valence shell diagrams.
Ca is what element?
Ar is what element?
Compare Ca to Ar:
Calcium Argon
Both have 3 full shells of electrons, 1s, 2s and 2p, 3s and 3p.Calcium has 2 more electrons in the 4s shell.
Previous
Ca: 1s22s22p63s23p64s2
Ar: 1s22s22p63s23p6
Cl: 1s22s22p63s23p5
What element is Cl? Draw its valence shell diagram.
Compare Cl to Ar:
Previous
Ca: 1s22s22p63s23p64s2
Ar: 1s22s22p63s23p6
Cl: 1s22s22p63s23p5
What will it take for calcium and chlorine to be like argon?
Why would calcium and chlorine want to be like argon?
Previous
K: 1s22s22p63s23p64s1
Ar: 1s22s22p63s23p6
Draw the valence shell diagrams.
What element is K?
Compare and contrast:
Why is argon stable?
How can K become “Noble Gas” like?
Previous
Ca: 1s22s22p63s23p64s2
Ga: 1s22s22p63s23p64s23d104p1
What element is Ga? Draw its valence shell diagram.
Compare and contrast:
Important
“Noble Gas Like” means to have a full octet of valence electrons in the s and p orbitals.
The atoms do not become Noble Gases.
Only the atomic number determines the name of the element. The only way to change to another element is nuclear decay, remember the proton and neutrons are in the nucleus not the electrons.
Chemical Bond
A chemical bond is the force that holds two atoms together.
One way is an attraction between the electron (-) on one atom and the nucleus of another (+).
Another way is the attraction between ions.
Group 1
Li: 1s22s1 or [He] 2s1
The outermost shell has 1 electron.
Remove 1 electron and lithium is like the Noble Gas helium, called lithium cation
Li1+
Group 1
Na: 1s22s22p63s1 or [Ne]3s1
The outermost shell has 1 electron.
Remove 1 electron and sodium is like the Noble Gas neon, called sodium cation
Na1+
Group 1
K: 1s22s22p63s23p64s1 or [Ar]4s1
The outermost shell has 1 electron.
Remove 1 electron and potassium is like the Noble Gas argon, called potassium cation
K1+
Group 2
Be: 1s22s12 or [He] 2s2
The outermost shell has 2 electrons.
Remove 2 electrons and beryllium is like the Noble Gas helium
Be2+
Group 2
Mg: 1s22s22p63s2 or [Ne]3s2
The outermost shell has 2 electrons.
Remove 2 electrons and magnesium is like the Noble Gas neon
Mg2+
Group 3
B: 1s22s2sp1 or [He] 2s22p1
The outermost shell has 3 electrons.
Remove 3 electrons and boron is like the Noble Gas helium
B3+
Transition Metals
Have full s2 orbitals
Lose these 2 electrons and maybe one electron in the d orbital
Sometimes it is difficult to predict how manyImportant to write cation symbol
Fe2+ and Fe3+
Anion
Negatively Charged Ion
Gain one or more electrons
Name is changed: __suffex becomes __ide
chlorine chloride
nitrogen nitride
Group 17
Flourine wants to be neon like.
Has 7 valence electrons and wants 8
Gains 1 electron and has a -1 charge
Flouride F-
Group 17
Chlorine wants to be argon like.
Has 7 valence electrons and wants 8
Gains 1 electron and has a -1 charge
Chloride Cl-
Group 17
Bromine wants to be krypton like.
Has 7 valence electrons and wants 8
Gains 1 electron and has a -1 charge
Bromide Br -
Group 16
Oxygen wants to be neon like
Has 6 valence electrons and wants 8
Gains 2 electron and has a -2 charge
Oxide O2-
Group 16
Sulfur wants to be argon like
Has 6 valence electrons and wants 8
Gains 2 electron and has a -2 charge
Sulfide S2-
Group 16
Write the Valance Electron Diagram for Selinium, Se
What noble gas does it want to be like?
How many electrons does it need?
Write the name and symbol for the anion.
Group 15
Find the number of valence electrons.
What noble gas do these elements want to be like?
Draw the electron dot structure for each.
Name the anion and write its name.
Nitrogen, Phosphorus and Arsenic
Formation of an AnionNotice“free’ electron
NoticeSmaller cloudNow Larger cloud
NoticeEnergy Released
Questions p. 209
1. Compare the stability of a lithium atom with that of its ion, Li+.
2. Describe two causes of the force of attraction in a chemical bond.
3. Why are all of the elements in group 18 unreactive, whereas those in group 17 are very reactive?
4. Summarize ionic bond formation by correctly paring these terms: cation, anion, electron gain, electron loss.
5. Write out the electron configuration for each atom. Then predict the change that must occur in each to achieve a noble-gas configuration.
a. nitrogen b. sulfur c. barium d. lithium
Fluorine
1. Write out electron configuration
2. Calculate number of valence electrons
3. What ion forms? (symbol)
4. What is the name of the ion?
Each Student
Write 5 element symbols on a piece of paper with atomic number 54 or lower.
Switch papersWrite electron configuration for each
elementDraw electron dot diagramDetermine what type of ion is most likely
formed