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Outcomes – January 30-Feb1

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- 1. Receive two mole bucks for having the practice quiz done priorto the quiz!
- 2. Revisit naming and formula writing, figuring out how to read the flow chart given
- 3. Learn what a mole is and why we use the unit “mole” to describe quantity of atoms and molecules!

- How many atoms of each element are in the reactants side of the following equation:
2 FeCl3 + 1 Be3(PO4)2 --> 3 BeCl2 + 2 FePO4

Now, do the same for the products side.

- What do you notice about the number of atoms?

- What is it called when the number and mass on both sides of the equation are equivalent to each other?

- Answer: The Law of Conservation of Mass

- Schedule a time with my teacher to re-take Unit 7 Quiz during Office Hours or Seminar, if I need to
- Be an ace at calculating molar mass for atoms and for compounds
- Write down that the Unit 8 Test is February 13 (A)-14 (B)

- 1. Which type of compound, ionic or covalent, do you use prefixes for?
- 2. What always goes first in the name of ionic compounds: the cation or the anion?
- 3. Write the molar mass for one mole of Tungsten, in grams
- 4. Write the formula: Magnesium chloride
- 5. How many atoms are in one mole of Carbon?
- 6. How many grams are in two moles of Na2SO4?

- You are expected to draw the conversions chart and to have your calculator in Chemistry class from now on!
- 1. How many moles of Hydrogen are in 28.9 grams of Hydrogen?
- 2. How many atoms of Germanium are in 4.2 moles of Germanium?
- 3. What must you sum up when calculating the molar mass of a compound?
- 4. If you have a coefficient of 2 for a compound, what happens to the total number of atoms for an element in the compound?

- 1. Learn how to calculate molar mass
- 2. Practice writing names and formulas for ionic and covalent compounds
- 3. Ace an exit quiz which tests your mastery of naming and formula writing and moles

- 1. Write the formula for lithium carbonate
- 2. How many atoms of each element are in: 4LiC2H3O2 and 4Mg3(SO4)2
- 3. Write the name for Si2O4
- 4. How many moles are in 36.03 particles of Carbon? (Hint: use 6.02x10^23 _______ = 1 mole ____)

Unit 8 – Moles, Types of reactions, balancing equations

- Determine the number of atoms in each of the following (ie: 1 carbon atom, 3 oxygen atoms, etc):
Li2SO4 Al(OH)3 N2O3

CCl4 Mg3(PO4)2 BeCl2

- Name them.

- Bell work
- The mole
- Practice with conversions
- Naming Challenge
- Homework: Molar mass and conversions homework

- Is anyone interested in joining honors for second semester?
- Pick up an application! The due date has been extended.

The mole and Molar Mass

- Quantity of particles
- Volume of gases at STP (Standard Temp and Pressure
- We’ll get to this later

- Mole to mole ratios
- Molar mass

Dozen = 12

Pair = 2

Names associated with an amount

Can you think of any more?????

- 1 mole = 6.02 x 1023 particles
- If I have a mole of M&Ms, how many M&Ms do I have?
- If I have a mole of pennies, how many pennies do I have?

The Mole

6.02 x 1023 atoms

6.02 x 1023

6.02 x 1023 Watermelon seeds would be found inside a melon slightly larger than the moon.

6.02 x 1023

6.02 x 1023 Donut holes would cover the Earth and be 5 miles deep.

HOLEY MOLEY!!!!

6.02 x 1023

6.02 x 1023 Pennies would make at least 7 stacks that would reach the moon.

6.02 x 1023

6.02 x 1023 Grains of sand would be more than all of the sand on Miami Beach.

6.02 x 1023

6.02 x 1023 Blood cells would be more than the total number of blood cells found in every human on Earth.

6.02 x 1023

A 1 Liter bottle of water contains 55.5 moles H2O.

6.02 x 1023

A 5 pound bag of sugar contains 6.6 moles of C12H22O11.

6.02 x 1023

There are 3 types of moles that live underground in North America: Eastern Mole, Hairy-Tailed Mole and Star-Nosed Mole.

The Mole

6.02 x 1023 atoms

6.02 x 1023 somethings = 1

- Atoms are very, very small.
- 1 atom of hydrogen weighs approximately 1.67 x 10-27 kg.
- As a result, it’s not very practical to do chemical reactions by counting out the number of atoms or molecules that will be reacting, because we’ll be counting for a very long time!

- You’ve seen this before, because when working with a large number of objects, it’s frequently handy to use units that are easier to work with.
- 2 shoes = 1 pair
- 12 eggs = 1 dozen
- 144 pencils = 1 gross
- 500 sheets of paper = 1 ream
- 6.02 x 1023 atoms or molecules = 1 mole
- The idea behind moles is the same as the idea behind “dozens”, except that the number is much bigger.

- Yes, we could.
- Although we could use moles to describe numbers of things that we work with everyday, it’s not really very practical.
- 1 mole of most objects that you work with on a daily basis is very, very large. For example, 1 mole of M&M’s would cover the continental United States to a depth of 125 km.

The Mole…..

The mole (mol) is the amount of a substance that

contains as many elementary entities as there

are atoms in exactly 12.00 grams of 12C

1 mol = NA = 6.0221367 x 1023

Avogadro’s number (NA)

eggs

- Mass of 1 mole of a compound
- Units: grams/mole (g/mol)

Molar mass is the mass of 1 mole of in grams

shoes

marbles

atoms

1 amu = 1 g/mol

These numbers are proportional

(how convenient!)

What is the mass of one mole of:

32.06 g/mol

S

C

12.01 g/mol

200.59 g/mol

Hg

Cu

63.55 g/mol

Fe

55.85 g/mol

3.2

- Sum the masses of all of the atoms in the molecule
- Example: NaCl
Na:22.99 grams x1 atom = 22.99 g/mol

Cl: 35.45 grams x 1 atom =35.45 g/mol

Total: 58.44 grams/mol

- Find the molar mass of Mg(NO3)2,
- MgCl2
- Fe(OH)2,
- Be3(PO4)2
Mg: 24.31 grams x 1 atom = 24.31 grams/mol

N: 14.01 grams x 2 atoms = 28.02 grams/mol

O:16.00 grams x 6 atoms = 96.00 grams/mol

Total: 148.33 grams/mol

- MgCl295.21 g/mol
- Fe(OH)290 g/mol
- Be3(PO4)2217 g/mol

- How do you count out a mole of atoms?
- You don’t. Even if it were possible to count out individual atoms in a reasonable period of time, the equipment we have only measures “grams.”
- As a result, we need to be able to convert between atoms/molecules, moles, and grams.

- 1 mole = _____ g (molar mass)
- 1 mole = 6.02 x 1023 atoms or molecules (Avogadro’s number)
- 1 always goes in front of moles!

grams

Molecules

or atoms

Molar

mass

6.02 x 1023

moles

- Convert as usual
- Handy hint:
- In conversion factors, always write “1” in front of “moles”!
- ******YOU MUST ALWAYS GO THROUGH MOLES!!!********

1 mol K

6.022 x 1023 atoms K

x

x

=

1 mol K

39.10 g K

How many atoms are in

0.551 g of potassium (K) ?

1 mol K = 39.10 g K

1 mol K = 6.022 x 1023 atoms K

0.551 g K

8.49 x 1021 atoms K

Let’s try a few more…………….

3.2

- How many grams are in 2.1 moles of Be?
- How many molecules are in 6.3 moles of CH4?
- How many molecules are there in 11.1 grams of carbon dioxide?
- How many grams are in 4.1 x 1023 molecules of H2O?

- How many grams are in 2.1 moles of Be? (18.9)
- How many molecules are in 6.3 moles of CH4? (3.79 x 1024 molecules)
- How many molecules are there in 11.1 grams of carbon dioxide? (1.51 x 1023 molecules)
- How many grams are in 4.1 x 1023 molecules of H2O? (18.7 g).

- Molar mass and conversions IP