chemical bonding and nomenclature - welcome! -...

Chemical Bonding and Nomenclature

By Paul Surko New Dimensions High School Poinciana, FL

November 30, 2016● Please hold on to

bonding worksheets from yesterday

● If I have yet to sign your SMART goals please turn them in along with your syllabus if I haven’t received it.

● We have a lot to review today, in order to do it I need your help!

● Friday cometh…..ready or not!

Bellwork: 1. What do you need from

me in order to succeed in this class?

2. What charge do atoms in group 1A and 7A take? What type of bond do they make? How do you know?

3. When would it be appropriate to draw a lewis structure?

4. How many electrons do ALL atoms want?

s

8BondChemical

I want you to meet a friend of mine?Bonding, the way atoms are attracted to each other to form molecules, determines nearly all of the chemical properties we see. And, as we shall see, the number “8” is very important to chemical bonding.

5.1 What are Molecules?Molecules are a

combination of atoms bonded together. Bonding determines the chemical

properties of the molecule (compound).

5.5 Ionic Bonding-Being Like the Noble Gases

All atoms want to have the same number of electrons as the Noble Gases. The Noble Gases have very stable electron configurations. In order to achieve the same electron configuration as the Noble Gases metal atoms will give up electrons to form positive ions (cations) and non-metal atoms will receive or take additional electrons to become negative ions (anions). IONS are charged particles.

N becomes N-3

Al becomes Al+3

Cl becomes Cl- O becomes O-2

Mg becomes Mg+2Na becomes Na+

The positive and negative ions are attracted to each other electrostatically.

Opposites Attract!

Putting Ions TogetherNa+ + Cl- = NaCl

Ca+2 + O-2= CaO Na+ + O-2 = Na2O

Al+3 + S-2 = Al2S3 Ca+2 + N-3 = Ca3N2

Ca+2 + Cl- = CaCl2

You try these!

Mg+2 + F- =

NH4+ + PO4

-3 =

K+ + Cl- =

Al+3 + I- =

Sr+2 + P-3 =

Li+ + Br- =

Sr3P2

AlI3

MgF2

(NH4)3PO4

KCl

LiBr

Not NH43PO4

December 1, 2016

1. What is your favorite holiday tradition (or winter tradition if you do not celebrate Christmas) ?

2. Draw the Lewis Structure for carbon disulfide

3. Write the chemical formula for Magnesium Bromide

5.2 The Covalent BondAtoms can form molecules by sharing

electrons in the covalent bond. This is done only among non-metal atoms.

5.3 Dot Structures-Octet Rule (All atoms want 8 electrons around them.)

Valence electrons are those in the outermost orbitals. They are the ones that can form bonds.

Lewis came up with a way to draw valence electrons so that the bonding could be determined.

Rules to Write Dot Structures1. Write a skeleton molecule with the lone atom in the middle (Hydrogen can never be in the middle) 2. Find the number of electrons needed (N) (8 x number of atoms, 2 x number of H atoms) 3. Find the number of electrons you have (valence e-'s) (H) 4. Subtract to find the number of bonding electrons (N-H=B) 5. Subtract again to find the number of non-bonding electrons (H-B=NB) 6. Insert minimum number of bonding electrons in the skeleton between atoms only. Add more bonding if needed until you have B bonding electrons. 7. Insert needed non-bonding electrons around (not between) atoms so that all atoms have 8 electrons around them. The total should be the same as NB in 5 above.

Let's Try it!1.S

2.N

3.H

4.B

5.NB

6.E .. H:O:H ●●

H O H Water H2O

2 x 2 = 4 for Hydrogen1 x 8 = 8 for Oxygen 4+8=12 needed electrons

8 – 4 = 4 non-bonding electrons

2 x 1 = 2 for Hydrogen1 x 6 = 6 for Oxygen You have 8 available electrons

12 - 8 = 4 bonding electrons

8 H12 N

4 B4 NB

-

-

H:O:H .. H:O:H ●●

Let's Try it!1.S

2.N

3.H

4.B

5.NB

6.E .. H:N:H ●●

H H N H Ammonia NH3

3 x 2 = 6 for Hydrogen1 x 8 = 8 for Nitrogen 6+8=14 needed electrons


3 x 1 = 3 for Hydrogen1 x 5 = 5 for Nitrogen You have 8 available electrons


8 H14 N

6 B2 NB

-

-

..H:N:H

.. H:N:H ●●

H

HH

Let's Try it!1.S

2.N

3.H

4.B

5.NB

6.E .. .. O::C::O●● ●●

O C O Carbon Dioxide CO2

1 x 8 = 8 for Carbon 2 x 8 = 16 for Oxygen 8+16=24 needed electrons


1 x 4 = 4 for Carbon 2 x 6 = 12 for Oxygen You have 16 available electrons


16 H24 N

8 B8 NB

-

-

O::C::O

.. .. O::C::O ●● ●●

Let's Try it!1.S

2.N

3.H

4.B

5.NB

6.E.. .. .. O::C: O: ●● ●●

OO C O Carbonate CO3

-2

3 x 8 = 24 for Oxygen 1 x 8 = 8 for Carbon 24+8=32 needed electrons


3 x 6 = 18 for Oxygen 1 x 4= 4 for Carbon You have 22 + 2 more available e-'s

24 H32 N

8 B16 NB

--

..O::C:O

.. .. .. O::C: O: ●● ●●

O

..:O: ..

:O:


-2

December 2, 2016

● Have your two worksheets out in front of you!

● Free write Friday write about whatever you want and then turn in your bellwork

● When you’re finished we’ll try a ticket out…..or in….lol the website is socrative.com and my room name is andie7216

http://socrative.com

5.6 Polarity-Unequal Sharing of Electrons

Even though all atoms want the same number of electrons as the Noble Gases, some want to get or give them more than others. The magnitude of this attraction for electrons is called “Electronegativity”. The more electronegative an atom is, the more it wants the electrons.

Some atoms want to gain electrons so bad, they take them altogether to form negative ions. Some want to lose them so bad that they become positive ions.

Examples of Polar and Non-Polar Compounds

H2O Water is a bent molecule. The lone pair of electrons from the Lewis structure distorts its shape and it becomes a very polar molecule.

NaCl Since Na is a metal it gives up its electron to form Na+ and Cl takes the electron completely to form Cl-.

HCl The Chlorine wants the electrons more than the Hydrogen. Thus we have +δHCl-δ.

Cl2 (Cl—Cl) The Chlorine molecules want the electrons equally so they form a non-polar molecule with NO partial or full charges.

CO2 Carbon Dioxide is a linear molecule. It has no lone pairs of electrons from the Lewis structure. The two oxygen atoms pull equally and make it a non-polar molecule.

.. :O:H ●● H

.. .. O::C::O●● ●●

5.7 NomenclatureNaming of Compounds

Binary Compounds have two types of atoms (not diatomic which has only two atoms).

Metals (Groups I, II, and III) and Non-Metals

Metal _________ + Non-Metal _________ideSodium Chlorine Sodium Chloride NaCl

Metals (Transition Metals) and Non-Metals

Metal ______ +Roman Numeral (__) + Non-Metal ________ide Iron III Bromine Iron (III) Bromide FeBr3 Compare with Iron (II) Bromide FeBr2

5.7 NomenclatureNaming of Compounds

Binary Compounds have two types of atoms (not diatomic which has only two atoms).

Metals (Transition Metals) and Non-Metals Older System

Metal (Latin) _______ + ous or ic + Non-Metal ________ide Ferrous Bromine Ferrous Bromide FeBr2 Compare with Ferric Bromide FeBr3

Non-Metals and Non-MetalsUse Prefixes such as mono, di, tri, tetra, penta, hexa, hepta, etc.

CO2 Carbon dioxide CO Carbon monoxide

PCl3 Phosphorus trichloride CCl4 Carbon tetrachloride N2O5 Dinitrogen pentoxide CS2 Carbon disulfide

Let’s Practice!Name the following.

CaF2K2SCoI2SnF2

SnF4OF2

CuI2CuISO2

SrSLiBr

Strontium SulfideLithium Bromide

Copper (I) Iodide or Cuprous IodideSulfur dioxide

Copper (II) Iodide or Cupric IodideOxygen diflourideTin (IV) Flouride or Stannic FlourideTin (II) Flouride or Stannous FlourideCobalt (II) Iodide or Cobaltous IodidePotassium SulfideCalcium Flouride

Acids (with H in front)Binary acids (without oxygen in formula)

Hydro _________ ic Acid

HCl Hydrochloric acid HBr Hydrobromic acid

Oxy acids (with oxygen in formula)

-ate goes to –ic and –ite goes to -ous

HNO3 Nitric acid HNO2 Nitrous acid H2SO4 Sulfuric acid H2SO3 Sulfurous acid H3PO4 Phosphoric acid H3PO3 Phosphorous acid

Lets Practice!HFNa2CO3

H2CO3

KMnO4

HClO4H2SNaOHCuSO4

PbCrO4

H2ONH3

Hydrooxic acid (no……just water)Nitrogen trihydride (no..just ammonia)

Copper (II) sulfate or Cupric sulfateLead (II) chromate or Plubous chromate

Sodium hydroxideHyrdogen sulfuric acidPerchloric acidPotassium permanganate

Sodium carbonateHydroflouric acid

Carbonic acid

chemical bonding and nomenclature - welcome! -...

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