1. Elements and Compounds2
Elements and Compounds 1

2. Chapter Goals Metals, Nonmetals, and Metalloids.
Monoatomic, Diatomic and Polyatomic Elements
Physical States of Elements
Luster, Malleability, Ductility, and Hardness of Elements
Groups, Rows, and Section Names
Ions
Ionic and Covalent Compounds
Repeating Units of Elements and Compounds
Chemical Formulas
Subatomic Particles
Atomic Number and Mass Number
Isotopes
Radioactivity
Atomic Mass

3. Metals, Nonmetals, and Metalloids
Elements to the left of the bold staircase on the periodic table are metals while thiose to the right are non-metals. Any elements on either side of the staircase are metalloids. Note that Al is considered a metal and not a metalloid and H is considered a non metal.

4. Metals, Nonmetals, and Metalloids

5. Chemical Particles
An atom is the smallest particle of an element that maintains its chemical identity through all chemical and physical changes.
Fundamental particles are the basic building blocks of atoms, they consist of electrons, protons, and neutrons.
A molecule is the smallest particle of a diatomic or polyatomic element or a compound that can have a stable independent existence.

6. Monoatomic, Diatomic, and Polyatomic Elements
Most elements exist as single atoms. These are mono atomic elements.
Only a few elements are made up of two or more atoms, so they consist of molecules.
Diatomic elements consist of 2 atoms. Polyatomic elements are made up of more than 2 atoms.

7. Monoatomic, Diatomic, and Polyatomic Elements
Fig. 1-3, p. 7

8. Monoatomic, Diatomic, and Polyatomic Elements
Fig. 1-4, p. 7

9. Physical State of Elements
All elements are solids at room temperature except:
a.) those that are liquids
(Hg and Br2)
b.) those that are gases

10. Luster, Malleability, Ductility and Hardness of Elements
Metals have luster. Nonmetals do not have luster, so they are dull.
Most metals are malleable (they can be rolled or hammered into shape).
Most metals are ductile (they can be drawn into wires).
Most metals are hard.
Nonmetals are neither malleable nor ductile.
Nonmetals are soft.

11. Group, Row, and Section Name of Certain Elements
In the periodic table, horizontal rows are referred to as periods.
Vertical columns are referred to as families.
Elements that are in certain groups, rows, and sections have specific names:
Group IA are the alkali metals.
Group IIA are the alkaline earth metals.
Group VIA are the chalcogens.
Group VIIA are the halogens.
Group VIIA are the noble gases.
The “B” group elements are the transition metals.
The two rows at the bottom of the periodic table are the lanthanides, or rare earth elements, and the actinides. Together they are called the inner transition metals.
Hydrogen is neither an alkali metal nor a halogen.

12. Group, Row, and Section Name of Certain Elements

13. Ions Elements can gain or lose electrons and become ions.
An ion is an atom or a group of atoms that carries and electrical charge.
A cation possesses a positive charge. e.g. Na+, Mg2+
An anion possesses a negative charge. e.g. Cl- , S2- .
A polyatomic ion is a group of atoms that bear an electrical charge. e.g. NH4+ (the only cation), SO42-, PO43-, OH-, NO3-.

14. Chemical Formulas
Chemical formula shows the chemical composition of the substance.
ratio of the elements present in the molecule or compound
He, Au, Na – monatomic elements
O2, H2, Cl2 – diatomic elements
O3, S8, P4 - more complex elements
H2O, C12H22O11 – compounds
Substance consists of two or more elements 4

15. Chemical Formulas Compound 1 Molecule Contains
HCl 1 H atom & 1 Cl atom
H2O 2 H atoms & 1 O atom
NH3 1 N atom & 3 H atoms
C3H8 3 C atoms & 8 H atoms 8

16. Ions and Ionic Compounds
Ions are atoms or groups of atoms that possess an electric charge.
Two basic types of ions:
Positive ions or cations
one or more electrons less than neutral
Na+, Ca2+, Al3+
NH4+ - polyatomic cation
Negative ions or anions
one or more electrons more than neutral
F-, O2-, N3-
SO42-, PO43- - polyatomic anions 9

17. Ions and Ionic Compounds
Sodium chloride
table salt is an ionic compound 9

18. Types and Basic Repeating Unit of Elements and Compounds
An atom is the smallest particle of an element that maintains its chemical identity through all chemical and physical changes.
Fundamental particles are the basic building blocks of atoms, they consist of electrons, protons, and neutrons.
A molecule is the smallest particle of an element or compound that can have a stable independent existence. It is incorrect to say a molecule of NaCl. The correct way is to indicate a formula unit of NaCl. It is also incorrect to say a molecule of He. You must say an atom of He. Examples of molecules include H2, S8, H2O, C6H12O6.

19. Types and Basic Repeating Unit of Elements and Compounds
Covalent
Monoatomic
Ionic
Type
Diatomic
Polyatomic
Basic
Repeating
Unit
Atoms
Molecules
Molecules
Formula
Unit
Molecule

20. Allotropes
Allotropes are different forms of the same element in the same physical state.
Examples: graphite and diamond are both C.
oxygen, O2, and ozone, O3, are
both O.

21. Allotropes
p. 48

22. Hydrates
A hydrate is a solid compound containing a definite percentage of bound water.
For example: CuF2 .2H2O
The heating of a hydrate results in the loss of bound H2O:
CuF2 .2H2O CuF2 + 2H2O D
This is considered a chemical change.

23. Subatomic Particles
Atoms are made up of even smaller particles called subatomic particles.
These subatomic particles are: electrons, protons, and neutrons.
There are other subatomic particles, but from a chemical perspective they are unimportant.

24. Subatomic Particles Particle Symbol Electrical Charge Approx. Mass
Proton p+ +1
1 amu
Neutron no
Electron e- -1
0 amu

25. Subatomic Particles
The following diagram depicts the arrangement of subatomic particles.
The nucleus, made up of protons and neutrons, is tiny in diameter
(approx Angstroms), yet heavy.
1 Angstrom (A) = 1 x m = 1 x 10-8 cm.
proton (p+)
10-15 m
Nucleus
neutron (no)
Electron (e-) Cloud
10-10 m

26. Subatomic Particles
Electrons are found outside the nucleus in certain energy levels.
In these levels the electrons are dispersed at a relatively great distance from the nucleus.
The diameter of an entire atom is in the range of 1-5 Angstroms.
The electrons are dispersed at distances that extend up to 105 times the diameter of the nucleus.

27. Subatomic Particles
Since like charges repel each other, that is why electrons are so far away from each other.
The nucleus, which contains protons (that have like charges) is very compact, however. The neutrons are said to be the glue that hold the protons together.
Like Charges Repel Each Other Opposite Charges Attract each other - + + - - +

28. Atomic Number (Z) and Mass Number (M)
The atomic number, Z, is what determines the atom’s identity.
Z = # of protons in an atom.
The atomic number for each element is found in the periodic table. Depending on the periodic table, the atomic number is either written below or above the element’s symbol. 18 Ar
39.95
39.95 Ar 18
Atomic Number

29. Atomic Number (Z) and Mass Number (M)
For atoms, # protons=# electrons. Therefore, atoms are electrically neutral.
For ions, # protons = # electrons.
Cations with a charge of c+ have c less electrons (but the same # of protons and neutrons) than its corresponding neutral atom.
Anions with a charge of (c-) have c more electrons (but the same # of protons and neutrons) than its corresponding neutral atom.
Being that electrons hardly weigh anything, the number of protons and neutrons that are present in a given atom is what essentially determines the mass of an atom.
Mass Number = # protons + # neutrons

30. Atomic Number (Z) and Mass Number (M)
What is the mass number, atomic number, and how many protons, neutrons, and electrons, that are present in the following species?
a.) mass number = 40, atomic number = 18
# protons = 18 = # electrons, # neutrons = = 22
b.)
c.) H+ 40 18 Ar
mass number = 32, atomic number = 16
# protons = 16, # electrons=18 # neutrons = 32-16=16 32 16
S2- 1
mass number = 1, atomic number = 1
# protons = 1, # electrons=0 # neutrons = 1-1 = 0

31. Isotopes
Isotopes are any two or more forms of an element having the same atomic number and the same chemical properties but different mass number and slightly different physical properties.
Isotopes of a given element have the same number of protons but different number of neutrons.

32. Isotopes
To distinguish between different isotopes of the same element we write an isotope symbol that indicates the mass number and the atomic number of the atom. The isotope symbol for one isotope of argon is:
Mass Number (M)
Symbol of
Element
Atomic Number (A)
M = # of p+ + # no
Z = # of p+
M-Z = [(#p+ + # no) - #p+) - #p+] = # of no

33. Isotopes
The following represents the arrangement of subatomic particles in an atom of Argon-40 (40 stands for the mass number):
Mass number = 40
# of p+ = 18
# of e- = 18
# of no = = 22
18 e-
18p+
22 no

34. Isotopes
Examples:
and are isotopes of the same element-Chlorine. ( atomic # = 17)
, (deuterium=D), and (tritium = T) are all isotopes.
Uranium-238 and Uranium-235 have different atomic masses (due to the different amount of neutrons) but chemically both would behave similarly.

35. Isotopes Example Problem:
Which of the following are isotopes of boron-12?
Only is an isotope.
Is boron-12, the identical atom.

36. Radioactivity
Elements with Z>83 are unstable (i.e., are radioactive).
Radioactivity is the spontaneous emission of high energy particles and/or radiation.
Radiation is the emission and transmission of energy through space in the form of waves.
Radioactive Substance is a substance that decays, or breaks down, spontaneously. They can decay by emitting one or more of the following: a) alpha particle, b) beta particle, c) gamma radiation.

37. Radioactivity Particles and Rays Frequently Encountered in Radiation:
Particle or ray
Name of radiation
Symbol
Charge
Biological Effects
Energetic Radiation
Gamma Ray
X Ray g
X-ray
Most penetrating, most damaging; can’t be stopped by shielding materials as easily as a and b particles.
Electron
Beta Particle
b or -1
Less penetrating than g-rays; not as harmful unless injested or inhaled.
Helium Nucleus
Alpha Particle
or a +2
least penetrating, not as harmful unless ingested or inhaled.

38. Atomic Mass (Weight) Scale
The atomic mass scale is based on the mass of the carbon-12 isotope. By definition all masses are determined relative to defining the mass of carbon-12 as exactly 12 amu.
Atomic masses (weights), found in the periodic table are not whole numbers because the weighted average of the masses of all the naturally occurring isotopes of the particular element is taken into account.
Since the mass of the electron is negligible compared to the mass of the nucleus, the atomic mass of an isotope is approximately equal to its mass number:
AW(average) = (f1 x AW1) + (f2 x AW2) + ….
where f1 = fraction of isotope #1
AW1 = atomic weight of isotope #1
f2 = fraction of isotope #2
AW2 = atomic weight of isotope #2

39. Atomic Mass Calculation
Calculate the average atomic mass of copper given the following information:
Isotope %Abundance Atomic Mass (amu)
63Cu
65Cu
AW(average) = (f1 x AW1) + (f2 + AW2)
f1 = 69.1 = f2 = 30.9 = .309
AW1 = AW2 = 64.9
AW(average) = (.691 x 62.9) + (0.309 x 64.9) = 63.6

40. Atomic Mass Calculation
Antimony has two common isotopes. If one of the isotopes is antimony-121 with an atomic mass of amu and an abundance in nature of 57.25%, what is the atomic mass (to 4 significant figures) of the other isotope?
From the periodic table we see that the average atomic mass for Sb is amu.
Since there are only two common isotopes, the % abundance of the second isotope is %-57.25% = 42.75%
AW(average) = (f1 x AW1) + (f2 + AW2)
= ( x ) + ( x AW2)
AW2 = – ( x ) = amu
.4275

41. Atomic Weight Calculation
The atomic weight of fictitious element X is amu. If element X consists of two isotopes that have mass numbers of 250 and 253, what is the approximate % natural abundance of each isotope?
Since the mass of the electron is negligible compared to the mass of the nucleus, the atomic weight of an isotope is approximately equal to its mass number.
Since there are only two isotopes, if one has an abundance of X the other isotope must have an abundance of 100%-X or in fractions 1-X.
Let X be the “fractional” abundance of 250X and (1-X) be the “fractional” abundance of 253X.
AW(average) = (f1 x AW1) + (f2 + AW2)
251.7 = [X x 250] + [(1-X) x 253]
251.7 = 250X – 253X
251.7 = -3X + 253
251.7 – 253 = X (Fraction of 250X) -3
Approx. abundance of 250X=43% and approximate abundance of 253X = 57%.