unit*3.*mole*unit*€¦ · chemistry 11 – mole concept study guide 1 avogadro’s number: •...
TRANSCRIPT
!!
Unit*3.*Mole*Unit*! Unit!conversions!involving!(HI!#4S7)*
o Atom,!molecule,!particle,!mole,!gram,!molarity,!density,!molar!mass,!volume,!gas!at!STP**
! Stoichiometry*
! !~ 15 classes 5 Quizzes (2 before break) 4 HIs 1 Formal Lab 1 Gum Lab 1 Unit Test
Chemistry 11 – Mole Concept Study Guide 1
Avogadro’s Number:
• There is a convenient unit when working with small particles such as atoms and molecules.
• This number is known as _________________, which is called __________________________, to honour the Italian scientist whose hypothesis led to its determination.
• If written out, this number looks like this:
602 000 000 000 000 000 000 000
Why do we need to know such a big number like this in Chemistry?
• Elements have different atomic masses (eg. Mg = 24.3g/mol, Ca = 40.1g/mol)
• Atoms and molecules are _____________ – we will work with _______ quantities of them.
• Need a convenient _____ to count atoms and molecules
• Example: A dozen ! instead of counting 1, 2, 3, we count by 12’s ! a known quantity that is understood by all. ! A convenient unit
• Chemists use a special term that is similar to “a dozen”.
• This term is called the “_________”
• 1 Mole is the same as having 6.02 x 1023 “things”
• Examples:
" 1 mole of Carbon atoms = 6.02 x 1023 Carbon atoms " 1 mole of Oranges = 6.02 x 1023 Oranges " 1 mole of Basketballs = 6.02 x 1023 Basketballs " 1 mole of Teachers = 6.02 x 1023 Teachers
• Notice in your comparisons that even though the ______ of a teacher is significantly
greater than the _______ of an orange, you will still get 6.02 x 1023 of them in a mole!
• Molar Mass: ___________________________________________________________.
" For an element, the molar mass is shown on the __________________________ " For a compound, it is the _____ of the atomic masses for each of the elements that
comprise it.
23
6. 02 X 10 Avogadro 's number
← to left 23 times
• y•
very small large
Unit" mole
"
moleuse mot as the unit w/ #
.
mass
mass
the mass of one mole of substance ( glmol )
periodic table eg ) carbon = 12.01
sum
Chemistry 11 – Mole Concept Study Guide 2
Molar Mass Calculation Notes
Step 1. Begin by separating out the different atoms found in the compound. H2O:
Step 2. Beside each atomic symbol, write how many are found in the compound. H2O: Step 3. Find the atomic mass of each atom and write the mass next to number corresponding to its element. H2O: Step 4. Multiply the atomic mass with the number of atoms of that element in the compound formula. H2O: Step 5. Add all totals to get the molar mass of the compound. H2O: Try these harder ones: (NH4)2SO4: Cu(NO3)2 • 6H2O:
Rule-
H When calculatingO
AutonsMM , Use IDP
.
H 2
O I
H 2 X 1.0 = 2 . O g
O I X 16.0 = 16.09
2. Og t 16.0g = 18.09
•
°
.MM ( Hz = 18.09 lmol
EIn Imol of H2O ,
you 'd weigh 18.0g .
→N 2 X 140 = 28.0
H 8 × 1- ° = & ° } SUM = 132. IpA m "
S 1 X 32.1 = 32- I
use IDP
O 4 X 16.0 = 64.0
6 6
If fun) copper # nitrate hexahydrateCU I x = 63.5
µ z ×
434.50= 28.0 } 295.591mm
O 12 X 16.0 = 192.0
H 12 × 1.0 = 12.0
Chemistry 11 – Mole Concept Study Guide 3
Diatomic Elements:
There are certain elements that exist as diatomic gas rather than single atom in nature. They are: Note:You must know these! To find molar mass of these gases, don’t forget to multiply the elemental molar mass by ___. Eg. Find the molar mass of hydrogen gas Molar Mass = Eg. Find the molar mass of chlorine gas Molar Mass =
HzIzBrzOzNzCkFz
2
um
H22.091mm
Eg .Find the MM of Chlorine Ton
.
urn me
Ck CI-
2X ( 35.5 )
= 71.091mg 35.59mmol
snow:{" ""
"
" "
?
?
⑧ Felt 17043-
ferric =
[email protected]'T } 357491mm
Sr ( OH)z
⑨SE
,I ¥9?! 8371 } in asana
Ionic Naz 5032 23.0 - 46 . O
Nga } ¥ 32 - I ÷ 32 - I } 126.191mm16.0 48.0
⑨-
Mg 3 Nz Ionic
Mn' 312*403 7%8 } 100.991mm