The document discusses the periodic table and periodic trends in properties of elements. It defines key periodic table terms like groups, periods, atomic radius, ionization energy, and provides examples of how properties change within periods and groups. It also discusses Mendeleev's original periodic table and the modern periodic law.

1. The Periodic Table

2. Periodic Vocabulary
 Atomic Radius  Metal
 Electronegativity  Metalloid
 Family  Noble Gas
 Group  Nonmetal
 Ionic Radius  Periodic Law
 Ionization Energy  Period

3. Classifying Elements
 Dmitri Mendeleev – observed that when
the elements were arranged in order of
increasing atomic mass, similar chemical
and physical properties appeared at
regular or periodic intervals.
 This was later determined to not exactly
be the case….
 Modern Periodic Law – The properties of
elements are periodic functions of their atomic
numbers.
◦ If the elements are arranged increasing atomic
number (not atomic mass) properties are repeated
periodically.
 For the majority of the table it is also appears as if it is
organized by increasing atomic mass, there are however some

4. Classifying Elements
 Dmitri Mendeleev – observed that when
the elements were arranged in order of
increasing atomic mass, similar chemical
and physical properties appeared at
regular or periodic intervals.
 This was later determined to not exactly
be the case….
 Modern Periodic Law – The properties of
elements are periodic functions of their atomic
numbers.
◦ If the elements are arranged increasing atomic number
(not atomic mass) properties are repeated periodically.
 For the majority of the table it is also appears as if it is organized
by increasing atomic mass, there are however some exceptions.
Can you spot them?
 Ar and K; Co and Ni; Te and I; Th and Pa, U and Np; Pu and Am; Lr and
Rf; Sg and Bh, Hs and Mi

5. Basic Periodic Table Info
Atomic
Mass Common oxidation
states (ions)
Chemical
Symbol
Atomic Number
Electron
configuration

6. Chemical Symbols
 Each symbol has one, two, or three letters.
◦ First letter is always capitalized.
◦ Other letters (if present) are lowercase.
C Au Uuu

7. Chemical Symbols
 Each symbol has one, two, or three letters.
◦ First letter is always capitalized.
◦ Other letters (if present) are lowercase.
C Au Uuu
Rg

8. Name the movie…

9. Arrangement of the Periodic
Table

10. Arrangement of the Periodic
Table
Metalloids
(semimetals)

11. General Characteristics of Element on the Periodic
Table
A. Metals: (Fr = most metallic element)
1. All (except Hg) are solid at room temperature.
2. Have luster. (are shiny)
3. Are Malleable (can be pounded into shape)
4. Are ductile (can be drawn into wires)
5. Are excellent conductors of heat and electricity.
 Due to mobile electrons.
6. Have low ionization energy.
Tend to lose electrons
7. Have low electro-negativity. and become postive (+)
ions.

12. General Characteristics of Element on the Periodic
Table
B. Nonmetals: (F = most nonmetallic)
1. Can be gases, liquids, or solids.
 Most nonmetals are gases or solids (molecular or
network) at room temperature.
 Bromine is a liquid at room temperature.
2. Lack luster. (are dull)
3. Are brittle. (crumble easily)
4. Are poor conductors of heat and electricity.
5. Have high ionization energy. Tend to gain electrons
6. Have high electro-negativity. and become negative (-)
ions.

13. General Characteristics of Element on the Periodic
Table
C. Metalloids: (semi-metals)
1. Properties are a combination of metallic and
nonmetallic substances.
 Located along the “staircase”
 B, Si, As, Sb, Te, Po

14. Elements in Nature
 Some elements can exist as a single atom
in nature, some cannot…
◦ Monotomic Elements: Most elements exist as
single atom particles in nature.
 Na, Si, Te, W
◦ Diatomic Elements: Some elements cannot
exist as a single atom, instead they exist as a
two atom particle in nature.
 HOFBrINCl’s
 H2, O2, F2, Br2, I2, N2, Cl2

15. Elements in Nature
◦ Allotropes: Some elements exist as two or
more forms in the same phase. These forms
differ in molecular or crystal structure, and hence
in their chemical and physical properties.
 Allotropes of Oxygen
◦ Oxygen (O2) and Ozone (O3)

16. Elements in Nature
 Allotropes of Carbon…
Coal/Graphite Diamon Buckminsterfulleren
d e
 Allotropes of Oxygen
◦ Oxygen (O2) and Ozone (O3)

17. Groups (Families)
 Vertical columns of elements.
◦ Have similar characteristics due to having
the same number of valence electrons.
 Example;
H
Li B F
Na Group 1 Al Group 13 Cl Group 17
K All have one Ga All have three Br All have seven
Rb valence In valence I valence
Cs electron. Ti electrons. At electrons.
Fr

18. Periods (rows)
 Horizontal rows of elements.
◦ Elements within a period have the same
number of occupied principal energy
levels.
 They differ however, in their chemical
properties.
Period 1: H, He use the 1st Principal Energy or… 1s
Level  Example;
Period 2: Li, Be, B, C, N, O, F, Ne use the 2nd Principal Energy
Level or…
1s2s2p
Period 3: Na, Mg, Al, Si, P, S, Cl, Ar use the 3rd Principal
Energy Level
or…

19. Trends in Properties
 Atomic Radius: (Table S)
◦ Covalent atomic radius: ½ the distance
between the nuclei of two atoms of the
same element joined in the solid phase by
a covalent bond.
 Within a period, atomic radius decreases.
 Within a family (group), atomic radius
increases.

20. Group Group Group Group Group
1 Li 2 B 3 C 4 O 5 Ne
e
Period
2
Period
Mg
3
Period
Ca
4

21. Trends in Properties
 Ionic Radius: (No Table/ Estimate using table
S)
◦ An atom that has gained or lost electrons,
will change in atomic size.
 Metals tend to lose electrons, thus the outer
shell is lost/pulled closer and the ionic radius
will be smaller than the covalent radius.
 Nonmetals tend to gain electrons, thus the
outer shell is stretched larger as the additional
electrons start to repel each other and the ionic
radius will be larger than the covalent atomic
radius.

22. Practice Question
 Which of the following has the greater
ionization energy, Na or Na+?
Explain your answer.

23. Practice Question
 Which of the following has the greater
ionization energy, Na or Na+?
Explain your answer.
Na+ has higher ionization energy as it
has 11 protons holding 10 electrons
while Na has 11 protons holding 11
electrons.

24. Summary
 Within a Period, as atomic number
increases.
1. Covalent atomic radius _______________
2. Ionization Energy _______________
3. Electronegativity _______________
4. Metallic Character _______________
 Within a group, as atomic number
increases.
1. Covalent atomic radius _______________
2. Ionization Energy _______________
3. Electronegativity _______________
4. Metallic Character _______________

25. Summary
 Within a Period, as atomic number
increases.
1. Covalent atomic radius decreases
Table S
2. Ionization Energy increases
3. Electronegativity increases Periodic Table
4. Metallic Character decreases
 Within a group, as atomic number
increases. Table S
1. Covalent atomic radius increases
2. Ionization Energy decreases Periodic Table
3. Electronegativity decreases
4. Metallic Character increases

26. Do Now
 Mendeleev arranged the periodic table in
orders of increasing atomic masses.
Locate iodine and tellurium on the table and
note that they are not arranged by
increasing atomic mass, and yet Mendeleev
placed iodine in Group 17 and tellurium in
Group 16. What is the likely reason that he
chose not to arrange these two elements by
atomic mass as he did for the majority of his
original table?

27. Do Now
 Mendeleev arranged the periodic table in
orders of increasing atomic masses.
Locate iodine and tellurium on the table and
note that they are not arranged by
increasing atomic mass, and yet Mendeleev
placed iodine in Group 17 and tellurium in
Group 16. What is the likely reason that he
chose not to arrange these two elements by
atomic mass as he did for the majority of his
original table?
He placed the tellurium and iodine into the
columns of elements with similar
characteristics.

28. Chemistry of Groups
Alkali Metals Alkali Earth
(1) Metals (2)

29. Chemistry of Groups
 Group 1
◦ Alkali Metals
 Have one valence electron. Form +1 ions.
(complete octet)
 Highly reactive.
 Reactivity increases as one proceeds from top to
bottom of the table (increasing atomic number).
 Typically form very stable compounds.
 Group 2
◦ Alkali Earth Metals
 Have two valence electrons. Form +2 ions.
(complete octet)
 Highly reactive.
 Reactivity increases as on proceeds from top to
bottom of the table (increasing atomic number).
Group 1 and Group 2 element are generally found as compounds in
 Typically only very stable compounds.
nature, and usuallyformseparated into elemental form by a process

30. Chemistry of Groups
*
*
“Staircase
” * *
* *

31. Chemistry of Groups
 Group 13,14,15,16
◦ “Staircase”
 Have 3,4, 5, and 6 valence electrons
respectively.
 Group 13 forms +3 ions. (Complete octet)
 Groups 14, 15, and 16 tend to gain e- and form -4, -3,
and -2 ions repectively. (Complete octet)
 Properties change from nonmetals (C/N) to
metalloids (Si/As) to metals (Pb/Bi) with
increasing atomic number.
Metals Metalloids Nonmetals
13 14 15 16 13 14 15 16 13 14 15 16
B C N O B C N O B C N O
Al Si P S Al Si P S Al Si P S
Ga Ge As Se Ga Ge As Se Ga Ge As Se
In Sn Sb In Sn Sb In Sn Sb
Te Te Te

32. Chemistry of Groups
The Halogens

33. Chemistry of Groups
 Group 17
◦ Halogens
 Have 7 valence electrons.
 Form -1 ions. (complete octet)
 Highly reactive nonmetals.
 Reactivity decreases with increasing atomic #.
 Halogen States of Matter (Room Temperature)
 F and Cl = gases
 Br = liquid
 I = solid
 At = No known stable isotopes. This means that all of its
isotopes are radioactive.
 *** All elements with an atomic number above 83 have
no known stable isotopes.***

34. Practice Question
 Why does chemical reactivity increase from
top to bottom of Group 1, while it decreases
from top to bottom of Group 17?

35. Practice Question
 Why does chemical reactivity increase from top
to bottom of Group 1, while it decreases from
top to bottom of Group 17?
Group 1 contains metal which lose electrons
and have large atomic radii in order to have low
ionization energy and low electronegativity.
Atomic radius increases as you move from top
to bottom of a group.
Group 17 contains nonmetals which gain
electrons so smaller atomic radii is required for
high ionization energy and high
electronegativity.

36. Chemistry of Groups
Noble Gases

37. Chemistry of Groups
 Group 18
◦ Noble (Inert) Gases
 Have 8 valence electrons. (Complete Octet)
 Generally NOT reactive.
 *** Under extreme conditions Kr and Xe have been
made to react with Flouring and Oxygen. This is why
they have oxidation numbers other than 0.***

39. Chemistry of Groups
Transition Metals
d sublevel elements
Lanthanide Series
Actinide Series
f sublevel elements

40. Chemistry of Groups
 Groups 3 to 12
◦ Transition Metals
 Generally exhibit positive oxidation numbers.
 All contain electrons that are “bounced” between
two outer principal energy levels; as a result
these elements are usually in a constant semi-
excited state.
 Solutions of these elements are usually colorful.

41. Chemistry of a Period
 As one progresses from left to right along
the periodic table:
◦ There is a change from + to – oxidation states.
◦ There is a change in characteristics from:
Very Less Less Very Noble
Reacti Reacti Metalloi Reactive Reactive (Inert)
ve ve ds (Nonmetals (Nonmetals Gases
(Metal (Metal ) )
s) s)

42. Do Now
 Elements with atomic number 112 and 114 have
been produces and their IUPAC names are
pending approval. However, an element that would
be put between these two elements on the periodic
table has not yet been produced. If produced this
element will be identified by the symbol Uut until an
IUPAC name is approved.
◦ Determine the charge of the Uut nucleus. Include both the
numerical value and the sign of the charge.
◦ Identify one element that would be chemically related to
Uut.

43. Do Now
 Elements with atomic number 112 and 114 have
been produces and their IUPAC names are
pending approval. However, an element that would
be put between these two elements on the periodic
table has not yet been produced. If produced this
element will be identified by the symbol Uut until an
IUPAC name is approved.
◦ Determine the charge of the Uut nucleus. Include both the
numerical value and the sign of the charge.
+113
◦ Identify one element that would be chemically related to
Uut.
Any element of Group 13; B, Al, Ga, In, Tl

44. Using the Periodic Table to
predict Chemical Formulas
 Water (H2O) is formed by the sharing of
electrons so that each atom can try to
emulate the outer shell electron
configuration of a noble gas (complete
octet)
◦ Hydrogen (H) tries to be like Helium (He)
◦ Oxygen (O) tries to be like Neon (Ne)
Covalent
Bond
We will explore this further when we start to learn about

45. Using the Periodic Table to
predict Chemical Formulas
 Hydrogen belongs to Group 1 which form
+1 ions.
 Oxygen belongs to Group 16 which form -2
ions.
Nonmetal

46. Using the Periodic Table to
predict Chemical Formulas
 Ice melt (CaCl2) is formed by the electromagnetic
attraction between positive ions forms by a metal
and the negative ions formed by a nonmetal.
◦ Calcium (Ca) loses its 2 electrons to become the
Ca+2 ion in order to be like the Noble gas Argon
(Ar)
2-8-8-2 2-8-8
2-8-8
◦ Chlorine (Cl) gains an electron to becom the Cl-1
ion in order to be like Argon (Ar) as well.
2-8-8
2-8-7 2-8-8

47. Using the Periodic Table to
predict Chemical Formulas
Metal Nonmetal
Ionic
Bond

48. Using the Periodic Table to
predict Chemical Formulas
 Predict the chemical formulas for the following…
 K+1 P-3  Beryllium and Carbon
 Mg+2 Cl-1  Cesium and Fluorine
 Ca+2 S-2  Group 13 (X) and
Group 16 (M)
 B+3 O-2

49. Using the Periodic Table to
predict Chemical Formulas
 What would be the general formula of a
Group 2 element (represented by M)
combined with chlorine of Group 17?
 What would be the general formula of a
group 16 element (represented by X)
combined with sodium of group 1?

50. Using the Periodic Table to
predict Chemical Formulas
 In the 19th century, Dmitri Mendeleev
predicted the existence of a then unknown
element X with a mass of 68. He also
predicted thant an oxide of X would have
the formula X2O3 . On the modern periodic
table, what is the group number and period
number of element X.

51. Using the Periodic Table to
predict Chemical Formulas
 What groups do the elements of the folwing
compound belong to?
◦ Mg3P2
◦ AlBr3
◦ GaN
◦ CH4

52. Isoelectricity
 Ions and atoms (noble gases) that
contain the same number of electrons.
◦ Example;
 K+1, S-2, and Ar are isoelectronic because they
each contain 18 electrons.
 Ge-4, Br-1, Rb+1, Sr+2, and Kr are
isonelectronic because they contain 36
electrons.

53. Practice question
 Ions are isoelectronic when they contain the same
number of electrons. Which of the following ions
are isoelectronic?
◦ Mg+2, Cl-1, Al+3, K+, S-2, Ba+2
 For each of the preceding ions name the nobles
gas with which they are isoelectronic with.

54. Metals and Conductivity.
 In terms of electrons, why are metals
good conductors of electricity?
◦ The valence electrons of metals are
mobile and form an electron “cloud”
around the metallic bonds of a given
metal element.
 This “cloud” of mobile electrons also serves in
the thermal conductivity of metals.

55. To get these slides go to…
http://mrmartinschemistryblog.blogspot.c
om