Contemporary phil. music music 10-q3

1. Module 2
Live
Discussion
Module 02 - Atoms and Molecules

2. What is your favorite holiday and
why?

3. Module 02 – Atoms &
Molecules
 By the end of this module you should be able to:
 Identify the components of atoms.
 Explain why different elements have different properties.
 Differentiate between the various trends illustrated by
the periodic table.
 Compare and contrast atoms and ions.
 Analyze molecules using chemical formulas and
structural formulas.
 Formulate the chemical formula of a compound from its
name.
 Give the name of a compound from its chemical formula.

4. Module 2 Assignments
Module 02 Lab 01 - Coffee Problem
Module 02 Lab 02 - Powerade
Module 02 Lab 03 - Periodic Table
He, C, O, Sb, Na, Si, Nb, Cl, K, Kr
Module 02 Assignment
Module 02 Quiz (36 questions)
Module 02 Live Classroom

5. Introduction to the Atom
 Atomic Mass Unit (amu) is the most common unit. It is
defined as one-twelfth of the mass of a carbon atom
containing six protons and six neutrons.
 Proton and Neutron Mass in SI Units
 Protons mass = SI unit =1.67262 x 10-27 kg = 1.0073 amu
 Neutrons mass = SI unit = 1.67493 x 10-27 kg = 1.0087
amu
 Electrons mass = SI unit = 0.00091 x 10-27 kg = 0.00055
amu

6. Periodic Table

7. Element Information

8. Elements
Atomic Number
Chemical Symbol
Mass (Protons & Neutrons)
For any element:
Number of Protons = Atomic Number
Number of Electrons = Number of Protons = Atomic Number
Number of Neutrons = Mass Number - Atomic Number
For krypton:
Number of Protons = Atomic Number = 36
Number of Electrons = Number of Protons = Atomic Number = 36
Number of Neutrons = Mass Number - Atomic Number = 84 - 36 = 48

9. Elements
Atomic Number
Chemical Symbol
Mass (Protons & Neutrons)

10. Isotopes

11. Isotopes

12. Atomic Mass
 An atomic mass (symbol: ma) is the mass of a single
atom of a chemical element. It includes the masses of the
3 subatomic particles that make up an atom: protons,
neutrons and electrons. ... 1 atomic mass unit is defined
as 1/12 of the mass of a single carbon-12 atom.
Example: You are given a sample containing 98% carbon-12
and 2% carbon-13. What is the relative atomic mass of the
element?

13. Atomic Mass
First, convert the percentages to decimal values by dividing each
percentage by 100. The sample becomes 0.98 carbon-12 and
0.02 carbon-13. (Tip: You can check your math by making certain
the decimals add up to 0.98 + 0.02 = 1.00).
Next, multiply the atomic mass of each isotope by the proportion
of the element in the sample:
0.98 x 12 = 11.76
0.02 x 13 = 0.26
For the final answer, add these together:
11.76 + 0.26 = 12.02 g/mol

14. Element Groups

15. Element Groups
The alkali metals are the series of elements in Group 1 of the
periodic table (excluding hydrogen in all but one rare circumstance).
The series consists of the elements lithium (Li), sodium (Na), potassium (K), rubidium (Rb),
caesium (Cs), and francium (Fr).
The alkaline earth metals are the series of elements in Group 2 of the periodic table.
The series consists of the elements beryllium (Be), magnesium (Mg), calcium (Ca), strontium (Sr),
barium (Ba) and radium (Ra) (though radium is not always considered an
alkaline on earth due to its radioactivity).
The halogens are the elements in Group 17 (formerly Group VII or VIIa) of the periodic table.
They are fluorine (F), chlorine (Cl), bromine (Br), iodine (I), astatine (At)
The carbon group is the series of elements in group 14 [formerly group IV) in the
periodic table.
It consists of the elements carbon (C), silicon (Si), germanium (Ge), tin (Sn), lead (Pb), and
ununquadium (Uuq).

16. Electron Configuration
In atomic physics and quantum chemistry, the electron
configuration is the distribution of electrons of an atom
or molecule (or other physical structure) in atomic or
molecular orbitals. For example, the electron
configuration of the neon atom is 1s2
2s2
2p6
,

17. Electron Configuration

18. Mass Ratio
Calculate the mass ratio of sulfuric acid, H2SO4.
H2SO4 contains hydrogen (H), sulfur (S), and oxygen (S).
From the periodic table, you can see that the molar masses of
these elements are:
H = 1.00
S = 32.06
O = 16.00

19. Answer
 There are two H atoms present, one S atom and four O atoms, so you have:
 H = (2)(1.00 g) = 2 g
 S = (1)(32.06 g) = 32.06 g
 O = (4)(16.00 g) = 64 g
 Step 2: Determine the Molar Mass of the Compound
 Add together the figures you calculated in Step 2:
 2 + 32.06 + 64 = 98.06 g
 Step 3: Divide the Mass of Each Element Present by the Molar Mass
 This means dividing the individual masses from Step 1 by the result of Step 2.
 For H, you have 2 ÷ 98.06 = 0.0204 = 2.04 percent hydrogen
 For S, you have 32.06 ÷ 98.06 = 0.3269 = 32.69 percent sulfur
 For O, you have 64 ÷ 98.06 = 0.6527 = 65.27 percent oxygen

20. Module 2 Assignments

21. Module 2 Example Problems
Find the atomic number (Z) for each element.
A. Fr
B. Kr
C. Pa
D. Ge
E. Al
List the symbol and atomic number of each element.
A. Boron
B. Neon
C. Silver
D. Mercury
E. Curium

22. Module 2 Example Problems
Find the atomic number (Z) for each element.
A. Fr = 87
B. Kr = 36
C. Pa = 91
D. Ge = 32
E. Al = 13

23. Module 2 Example Problems
List the symbol and atomic number of each element.
A. Boron = B (5)
B. Neon = Ne (10)
C. Silver = Ag (47)
D. Mercury = Hg (80)
E. Curium = Cm (96)

24. Module 2 Example Problems
Copper has two naturally occurring isotopes: Cu-63 with
mass 62.9395 amu and a natural abundance of 69.17%,
and Cu-65 with mass 64.9278 amu and a natural
abundance of 30.83%. Calculate the atomic mass of
copper.

25. Module 2 Example Problems
Solution:
fraction Cu 63 = 69.17/100 = 0.6917
fraction Cu-65 = 30.83/100 = 0.3083
atomic mass = (0.6917 × 62.9395 amu) + (0.3083 ×
64.9278 amu)
= 43.5353 amu + 20.0172 amu = 63.5525 amu = 63.55
amu

26. Module 2 Example Problems
1. Find the number of protons and electrons in the O2-
ion.
2. Determine the charge of a selenium ion with
36 electrons.

27. Module 2 Example Problems
Solution:
1. The atomic number of O is 8; therefore, it has 8 protons.
Ion charge = # p+
- # e-
- 2 = 8 - # e-
# e-
= 8 + 2 = 10
2. Selenium is atomic number 34; therefore, it has 34
protons.
Ion charge = 34 – 36 = 2–

28. Module 2 Example Problems
1. How many protons and neutrons are in 62
28Ni?
Solution
The number of protons is equal to
Z (lower left number)
The number of neutrons is equal to
A (upper left number) - Z (lower left
number)
#n = 62 – 28 = 34 neutrons

29. Quiz Week 2
36 Questions
- Atomic Numbers and Symbols
- Electrons, Valance Electrons and Charges
- Protons, electrons, neutrons…
- Atomic Mass
-Groups on the periodical Table
- Wavelengths
- Electron Configuration
- Valance Electrons
- Periodical Table (atomic size)
- Mass Ratios
- Formulas and naming

30. Question
s?