1. Chapter 2 Atoms and Elements

2. Sources of Some Element Names
Some elements are named for planets, mythological figures, minerals, colors, scientists, and places.
A symbol
represents the name of an element.
consists of 1 or 2 letters.
starts with a capital letter
With few elements use their own special symbols
1-Letter Symbols 2-Letter Symbols
C carbon Co cobalt
N nitrogen Ca calcium
S sulfur Au gold Mg magnesium

3. Nonmetals: Right side of the zigzag line in the periodic table
Metals: Left side of the zigzag line in the periodic table (except for hydrogen)
Nonmetals: Right side of the zigzag line in the periodic table
Semimetals (metalloids): Tend to lie along the zigzag line in the periodic table
Dang

4. Transition Metals: 3B–2B (8 groups, 10 columns)
Main Groups
Columns 1A–2A (2 groups)
Columns 3A–8A (6 groups)
Transition Metals: 3B–2B (8 groups, 10 columns)
Inner Transition Metals: 14 groups between 3B and 4B
Lanthanides
Actinides
Dang

5. Law of Conservation of Mass
in a chemical reaction, matter is neither created nor destroyed
total mass of the materials you have before the reaction must equal the total mass of the materials you have at the end
total mass of reactants = total mass of products
7.7 g Na g Cl  g NaCl

6. Conservation of Mass and the Law of Definite Proportions
Chemistry: McMurry and Fay, 6th Edition
Chapter 2: Atoms, Molecules, and Ions
Conservation of Mass and the Law of Definite Proportions
2/16/ :00:43 AM
Law of Definite Proportions (John Dalton )
Different samples of a pure chemical substance always contain the same proportion of elements by mass.
Compound always forms from a fixed ratio of its element
How many Hydrogen atoms are there?
How many Oxygen atoms are there?
What is the ratio between Hydrogen atoms to Oxygen atom?
Now using the mass of Hydrogen and Oxygen to show these results are consistent with the law of definite proportion
Copyright © 2011 Pearson Prentice Hall, Inc.

7. Proportions in Sodium Chloride
a g sample of sodium chloride contains 39.3 g of sodium and 60.7 g of chlorine
a g sample of sodium chloride contains 78.6 g of sodium and g of chlorine
a g sample of sodium chloride contains g of sodium and g of chlorine

8. The Law of Multiple Proportions and Dalton’s Atomic Theory
Chemistry: McMurry and Fay, 6th Edition
Chapter 2: Atoms, Molecules, and Ions
The Law of Multiple Proportions and Dalton’s Atomic Theory
2/16/ :00:43 AM
Law of Multiple Proportions: If two elements (A and B) form more than one compound (AB, AB2, AB3 …) then the ratios of the masses of the second element which combine with a fixed mass of the first element will be the ratio of small whole number
- Show how chemical formulas are put together
nitrogen monoxide (NO):
nitrogen dioxide (NO2):
7 grams nitrogen per 8 grams oxygen
7 grams nitrogen per 16 grams oxygen
Insert Figure 2.2 p37
Copyright © 2011 Pearson Prentice Hall, Inc.

9. Example Lead forms two compounds with oxygen as shown:
PbO: g Pb, g O
PbO2: g Pb, g O
Show these results consistent with the law of multiple proportions

10. Dalton’s Atomic Theory
Dalton proposed a theory of matter based on it having ultimate, indivisible particles to explain these laws
Each element is composed of tiny, indestructible particles called atoms
All atoms of a given element has the same mass and other properties that distinguish them from atoms of other elements
Atoms combine in simple, whole-number ratios to form molecules of compounds
In a chemical reaction, atoms of one element cannot change into atoms of another element
they simply rearrange the way they are attached

11. J.J. Thomson (1897)
believed that the cathode ray was composed of tiny particles with an electrical charge
designed an experiment to demonstrate that there were particles by measuring the amount of force it takes to deflect their path a given amount
like measuring the amount of force it takes to make a car turn
anode
cathode 11

12. - Thomson’s Experiment ------------- anode cathode +
investigate the effect of placing an electric field around tube
(1) charged matter is attracted to an electric field
(2) light’s path is not deflected by an electric field
cathode
anode
(+)
(-) -
Power Supply +

13. Thomson’s Results the cathode rays are made of tiny particles
these particles have a negative charge
because the beam always deflected toward the + plate
Particles that make cup cathode rays are 2,000 times smaller than a Hydrogen
the amount of deflection was related to two factors, the charge and mass of the particles
every material tested contained these same particles
the only way for this to be true is if these particles were pieces of atoms
apparently, the atom is not unbreakable

14. Millikan’s Oil Drop Experiment
Millikan's experiment involved measuring the force on oil droplets in a glass chamber sandwiched between two electrodes, one above and one below. With the electrical field calculated, he could measure the droplet's charge,
the charge/mass of these particles was x 108 C/g
the charge/mass of the hydrogen ion is x 104 C/g

15. Thomson’s Plum Pudding Atom
The Plum Pudding Atom
the mass of the atom is due to the mass of the electrons within it
electrons are the only particles in Plum Pudding atoms
the atom is mostly empty space
cannot have a bunch of negatively charged particles near each other as they would repel
the structure of the atom contains many negatively charged electrons
these electrons are held in the atom by their attraction for a positively charged electric field within the atom
there had to be a source of positive charge because the atom is neutral
Thomson assumed there were no positively charged pieces because none showed up in the cathode ray experiment

16. Rutherford’s Results Over 98% of the a particles went straight through
About 2% of the a particles went through but were deflected by large angles
About 0.01% of the a particles bounced off the gold foil
“...as if you fired a 15” cannon shell at a piece of tissue paper and it came back and hit you.”

17. go through, but are deflected•
Plum Pudding
Atom
if atom was like
a plum pudding,
all the a particles
should go
straight through
a few of the
a particles
do not go through .
Nuclear Atom
most a particles
go straight through
some a particles
go through, but are deflected

18. Rutherford’s Interpretation – the Nuclear Model
The atom contains a tiny dense center called the nucleus
the amount of space taken by the nucleus is only about 1/10 trillionth the volume of the atom
The nucleus has essentially the entire mass of the atom
the electrons weigh so little they give practically no mass to the atom
The nucleus is positively charged
the amount of positive charge balances the negative charge of the electrons
The electrons are dispersed in the empty space of the atom surrounding the nucleus

19. Structure of the Atom
Rutherford proposed that the nucleus had a particle that had the same amount of charge as an electron but opposite sign
based on measurements of the nuclear charge of the elements
these particles are called protons
charge = x 1019 C
mass = x g
since protons and electrons have the same amount of charge, for the atom to be neutral there must be equal numbers of protons and electrons

20. Some Problems
How could beryllium have 4 protons stuck together in the nucleus?
shouldn’t they repel each other?
If a beryllium atom has 4 protons, then it should weigh 4 amu; but it actually weighs 9.01 amu! Where is the extra mass coming from?
each proton weighs 1 amu

21. There Must Be Something Else There!
to answer these questions, Rutherford proposed that there was another particle in the nucleus – it is called a neutron
neutrons have no charge and a mass of 1 amu
mass = x g
slightly heavier than a proton
no charge

22. Atomic Structure: Protons and Neutrons
The charge of the proton is opposite in sign but equal to that of the electron.
The mass of the atom is primarily in the nucleus.

23. Elements each element has a unique number of protons in its nucleus
the number of protons in the nucleus of an atom is called the atomic number
the elements are arranged on the Periodic Table in order of their atomic numbers

24. Structure of the Nucleus
Soddy discovered that the same element could have atoms with different masses, which he called isotopes
The observed mass is a weighted average of the weights of all the naturally occurring atoms
the percentage of an element that is 1 isotope is called the isotope’s natural abundance

25. Isotopes all isotopes of an element are chemically identical
undergo the exact same chemical reactions
all isotopes of an element have the same number of protons
isotopes of an element have different masses
isotopes of an element have different numbers of neutrons
isotopes are identified by their mass numbers
protons + neutrons
Atomic Number
Number of protons Z
Mass Number
Protons + Neutrons
Whole number A
Abundance = relative amount found in a sample

26. Examples
1. How many protons, electrons and neutrons are present in an atom of 2. Write isotopic symbols in both forms for Selenium isotope with 40 neutrons 3. An atom has 32 electrons and 38 neutrons. What is its mass number and what is the element?

27. Mass Spectrometry
masses and abundances of isotopes are measured with a mass spectrometer
atoms or molecules are ionized, then accelerated down a tube
their path is bent by a magnetic field, separating them by mass
similar to Thomson’s Cathode Ray Experiment
a mass spectrum is a graph that gives the relative mass and relative abundance of each particle
relative mass of the particle is plotted in the x-axis
relative abundance of the particle is plotted in the y-axis

28. Atomic Mass
we previously learned that not all atoms of an element have the same mass
isotopes
we generally use the average mass of all an element’s atoms found in a sample in calculations
we call the average mass the atomic mass

29. Atomic Masses and the Mole
The mass of 1 atom of carbon-12 is defined to be 12 amu.
Atomic Mass: The weighted average of the isotopic masses of the element’s naturally occurring isotopes
Carbon-12 is the only one that is exact. All others are done with respect to carbon-12. Since the element is made up of a number of isotopes in addition to carbon-12, the atomic mass of the element is a bit more than 12 amu.

30. Atomic Masses and the Mole
Why is the atomic mass of the element carbon amu?
Carbon-12: 98.89% natural abundanc e 12 amu
Carbon-13: 1.11% natural abundance amu
Mass of carbon = (12 amu)(0.9889) + ( amu)(0.0111)
= amu amu
= amu

31. Example
Lithium has two naturally occurring isotopes: lithium-6 and lithium-7. If the average atomic mass of lithium is amu, which isotope is the most abundant? How do you know?

32. Example
Natural occurring chlorine consists of 75.77% Cl-35 (mass amu) and 24.33% Cl-37 (mass amu). What is the atomic mass of Chlorine?

33. Collection Terms A collection term states a specific number of items.
1 dozen donuts
= 12 donuts
1 ream of paper
= 500 sheets
1 case = 24 cans
In chemistry, how do chemists know the number of atoms in an element or compound?

34. A Mole of Atoms
A mole is
a unit of measurement used in chemistry to express amounts of a chemical substance, the same number of particles as there are carbon atoms in 12.0 g of carbon.
a collection term “dozen”
1 mole = NA = x 1023 of anything
Avogadro’s Number = x 1023

35. Relationship Between Moles and Mass
The mass of one mole of atoms is called the molar mass
The molar mass of an element, in grams, is numerically equal to the element’s atomic mass, in amu
E.g 1 H atom = 1.01 amu
1 mol H = 1.01g
6.022 x atoms of H = ???? g

36. Examples Give the molar mass for each
A. 1 mole of Li atoms = ________ g
1 mole of Co atoms = ________g
1 mole of S atoms = ________g

37. Converting between mass, moles and atoms
g C
mol C
mol C
g C
g C
mol C
atoms

38. Examples
Assuming all pennies are pure copper and each has a mass of 2.5 g
Without doing calculation, determine the number atoms of copper present in 1 mole
How many pennies does it take to make a mole?

39. Examples
Calculate the moles and how many atoms of carbon in g of pencil lead
Calculate the mass (in grams) of moles of titanium

40. Example
If 2.26 x atoms of element X have a mass of 1.50, what is the identity of X?