chapter 3.3. objectives 1. explain what isotopes are 2. define atomic number and mass number, and...
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COUNTING ATOMSChapter 3.3
Objectives1. Explain what isotopes are2. Define atomic number and mass number,
and describe how they apply to isotopes.3. Given the identity of a nuclide, determine
its number of protons, neutrons, and electrons.
4. Define mole in terms of Avogadro’s number, and define molar mass.
5. Solve problems involving mass in grams, amount in moles, and number of atoms of an element
Atomic Number Symbol – Z Number of protons in nucleus of atom Determines the identity of the
atom!!!!! C - 6 He - ___ F - ___ Pb - ___
Use periodic table to find these! Since atoms are neutral atomic number is
also number of electrons So C also has 6 electrons He - ____ electrons
2
82
9
2
Isotopes All Hydrogen atoms contain 1 proton Many naturally occurring elements
can contain different numbers of neutrons.
Isotope – at0ms of the same element that have different masses.
n
Protium 99.985 %
Deuterium 0.015 %
Tritium Trace
Three isotopes of Hydrogen
nn
Mass Number Mass number – total number
of protons and neutrons in the nucleus of an isotope
Symbol – A Protium has 1 proton and 0
neutrons Mass number = #p + #n = 1 + 0 = 1
What is the mass number deuterium and tritium?
Find on periodic table
Designating Isotopes Hyphen Notation
Name of atom – mass number Uranium - 235
Nuclear symbol A
X A : mass number, Z : atomic number, X : symbol of element
235U92
Z
Nuclide – general term for any isotope of any element
Number of protons Neutrons Electrons
92 9214
3
Sample Problem A How many protons, electrons, and
neutrons are there in an atom of chlorine-37? atomic number = number of protons =
number of electrons mass number = number of neutrons +
number of protons # protons # electrons #neutrons
17Atomic number from periodic table
17 # protons = # electrons20Mass # = # protons + # electrons
Practice Pg. 801. How many protons, electrons, and
neutrons make up an atom of bromine-80?
2. Write the nuclear symbol for carbon-13.
3. Write the hyphen notation for the isotope with 15 electrons, and 15 neutrons.
Answer : 35 protons, 35 electrons, 45 neutrons
Answer : 13 C6
Answer : phosphorus – 30
Relative Atomic Mass Oxygen – 16 , mass of 2.657 x 10-23 g Easier to use relative scale
Need arbitrarily chosen standard All others are compared to carbon - 12
One atomic mass unit (1 amu) – exactly 1/12 the mass of a carbon – 12 atom.
All others are compared to carbon -12 Hydrogen – 1 , about 1/12 the mass of carbon -12
Precise value is 1.007825 amu
Magnesium – 24 , Slightly less than twice that of carbon -12• Precise value is 23.985042 amu
Average Atomic Mass of Elements Most elements occur naturally as
mixtures of isotopes Average atomic mass : weighted
average of the atomic masses of the naturally occurring isotopes of an element
Ex. of weighted average Box contains two types of marbles, 25%
have mass of 2.00g, and 75% have a mass of 3.00 g. 25 marbles x 2.00 g = 50 g 75 marbles x 3.oo g = 225 g so 50 g + 225 g = 275 g (TOTAL MASS)
275 g ÷ 100 = 2.75 g average marble mass
Calculating average atomic mass Or
(2.00 g x 0.25) + (3.00 g x .75) = 2.75 g Calculate the average atomic mass of copper
Use table 3-4 pg. 80 in text Copper - 63 69.17% with mass of 62.929599 amu Copper – 65 30.83% with mass of 64.927793 amu
(0.6917 x 62.929599 amu) + (0.3083 x 64.927793 amu)
=63.55Match with atomic mass on periodic table
Round to two decimal places in calculations Visual Concept – Click
Here
Relating Mass to Numbers of Atoms The MOLE
SI base unit for amount of a substance Abbreviated as mol Defined as : amount of substance that
contains as many particles as there are atoms in exactly 12 g of carbon – 12
Counting unit just like a dozen We don’t order 12 or 24 eggs, we order 1
or 2 dozen In same way, a chemist may want 1 mol of
carbon or 2 mol of iron.63.55 g of copper or 1 mol of copper
Visual Concept – Click Here
Avogadro’s Number The number of particles in a mole –
AVOGADRO’S NUMBER 6.022 x 1023 particles in exactly one
mole of a pure substance
How big is this number? If every person on earth (5 billion people)
counted 1 atom per second, it would take 4 million years to count all the atoms.
Visual Concept – Click Here
Molar Mass Molar mass – mass of one mole of a
pure substance Units : g/mol Numerically equal to atomic mass of
element Mass of 6.02 x 1023 atoms of element
One mole He 6.02 x 1023 atoms 4.oo g
One mole Li 6.02 x 1023 atoms 6.94 g
One mole Cu 6.02 x 1023 atoms 63.5o g
One mole Fe 6.02 x 1023 atoms 55.78 g
Visual Concept – Click Here
Gram/Mole Conversions
Mass In grams
Moles In mol
Atoms In atoms
Molar mass
Avogadro’s
Number
What is the mass in grams of 3.50 mol of the element copper, Cu?
Sample Problem B
3.30 mol Cu
x63.55 g Cu1 mol Cu
222 g Cu
=
Step 1:
Write the given value
Step 2:
Use molar mass from periodic table
Step 3:
Cancel out units
Step 4:
Calculate
Always round to 2 places after the decimal
Sample Problem CA chemist produced 11.9 g of Aluminum, Al. How many moles of aluminum were produced?
11.9 g Al
x26.98 g Al
1 mol Al
0.441 mol Al
=
How many moles of silver, Ag, are in 3.01 x 1023 atoms of silver?
Sample Problem D
3.01 x 1023 atoms Ag
x 0.500 mol Ag
1 mol Ag
=6.02 x 1023
atoms Ag
Avogadro’s number
Sample Problem EWhat is the mass in grams of 1.20 x 108 atoms of copper, Cu?
1.20 x 108atoms Cu
x
1.27 x 10-14 g Cu
1 mol Cu
=
6.02 x 1023 atoms Cu
x1 mol Cu
63.55 g Cu
Avogadro’s #
****Requires 2 conversions
Molar mass
The Ten Commolements
(found at http://members.tripod.com/~smalls42/commolements.html)
1. Thou shalt not use 6.02 x 1023 in vain. 2. Thou shalt not use the term mole if thou has no true
knowledge of the term mole. 3. Thou shalt not kill a mole. 4. Thou shalt not covet your neighbor's mole. 5. Thou shall always remember to celebrate Mole Day. 6. Thou shalt not disparage Mole Day. 7. Thou shalt not use a mole out of season. 8. Thou shalt always honor the one who introduced thou to Mole
Day. 9. You shalt always keep sacred 10/23. 10. Thou shalt always remember these commolments or thou will
never properly celebrate Mole Day.