1. THE PERIODIC TABLE

2. 2 Types of Chemistry
Organic Chemistry
Inorganic Chemistry

3. History of the Periodic Table
1871 – Mendeleev arranged the elements according to: 1. Increasing atomic mass Elements w/ similar properties were put in the same row
1913 – Moseley arranged the elements according to: 1. Increasing atomic number Elements w/ similar properties were put in the same column

4. Transitional Metals Lanthanide Series Actinide Series Noble Gases
Alkali Metals
METALLOIDS
Halogens
Alkaline Metals
Transitional
Metals
Lanthanide Series
Actinide Series

5. PERIOD- a row indicates the number of energy levels or electron shells.1 2 3 4 5 6 7

6. GROUP NUMBER- a column on the periodic table; also known as a family. IA
VIIIB
An alternate method:
IIA
IIIB
IVB VB
VIB
VIIB
IIIA
IVA VA
VIA
VIIA
VIIIA IB
IIB
GROUP NUMBER- a column on the periodic table; also known as a family.
Indicates how many electrons in the outer shell. All members of a family react similar to one another

7. PERIOD 1 1 2 3 PERIOD 2 4 5 PERIOD 3 6 7 PERIOD 4 PERIOD 5 PERIOD 6He
PERIOD 1 1 2 3 4 5 6 7 Fr
PERIOD 7 Rn
PERIOD 6 Xe
PERIOD 5 Ne
PERIOD 2 Kr
PERIOD 4 Ar
PERIOD 3

8. GROUP NUMBER- a column on the periodic table; also known as a family. 1 18 2 13 14 15 16 17 3 4 5 6 7 8 9 10 11 12
GROUP NUMBER- a column on the periodic table; also known as a family.
Indicates how many electrons in the outer shell. All members of a family react similarly to one another

9. Why are these elements grouped together?
Elements in the same family or group have similar chemial & physical properties...
GROUPS are columns of families

10. ALKALI METALS FAMILY In GROUP IA 2H2O + 2Na  2NaOH + H2 Lithium
1 valence electron
Lithium
Never found uncombined in nature.
2H2O + 2Na  2NaOH + H2
Reacts violently with water to form heat + Hydrogen gas + alkali (OH containing compound)
Sodium hydrogen
Hydroxide gas
Soft enough to cut with
a knife
Shiny.

11. ALKALINE EARTH METALS GROUP IIA Second most reactive metals.
Beryllium
Second most reactive metals.
Never found uncombined in nature.
Fairly hard.
Good conductors of electricity.
2 valence electrons
Magnesium + silver nitrate…
Magnesium alloy
Beryllium-Copper spring
Calcium in bones

12. TRANSITION METALS GROUPS IIIA Luster (shiny). Ductile. Malleable.
Metals or metal-like; 88 of them.
Good conductors of heat & electricity
1-3 valence electrons
Tends to lose valence electrons during bonding

13. METALLOIDS Found on both sides of zig zag line
Share properties of both metals & non-metals.
Dull or shiny.
Ductile ,malleable or mbrittle
Conducts heat & electricity, but not as well as metals.
Silicon
wafer
arsenic
silicon
tellurium

14. NON-METALS GROUPS IVB - VIIIB
17 elements located to the right of the zigzag line + Hydrogen
Gain or share valence electrons.
Physical properties are opposite metals.
Dull in appearance.
Poor conductors of heat and electricity
Readily form compounds (ie. H2O)
helium
Carbon (charcoal)
neon
Sulfur
krypton
iodine

15. HALOGENS GROUP VIIB HF HCl HBr All but one are non-metals.
7 valence electrons
Gain 1 electron when reacting with metals.
May share electrons when bonding with other non-metals (ie. CF4)
All are very reactive; usually harmful to humans.
Many acids contain halogens:
Rock containing
Fluorine
Iodine
Iodine
Chlorine
bleach HF
Hydrofluoric
acid
HCl
Hydrochloric
acid
HBr
Hydrobromic
acid

16. NOBLE OR INERT GASES GROUP VIIIB Chemically stable & non-reactive.
Have a filled outer shell (electrons)
Do not form compounds or react with other elements.
helium
neon
krypton

17. RARE-EARTH METALS plutonium neodymium uranium cerium
LANTHANIDES SERIES
Soft.
Malleable.
Good conductors.
Used to make alloys.
ACTINIDES SERIES
Metals.
Radioactive.
Nucleus very unstable.
Many are synthetic.
plutonium
neodymium
uranium
cerium

18. Which element is in a class by itself?
Why?
The answer is
Is it :
Hydrogen
Like Group 1:
It has 1 valence electron
Its most common isotope has no neutrons
Hydrogen
Helium
Gold
Platinum?
Unlike Group 1, it is a non metal.

19. Hydrogen Hydrogen Sun What is the Sun made of? <1% >99%
Therefore, what is the most abundant element in the Solar System?
Sun
>99% of All matter in the solar system is from the Sun.
<1% is everything else (planets, moons, comets, asteroids, etc)

20. Periodic Trends
Periodic Trends – patterns (don’t always hold true) can be seen with our current arrangement of the elements (Moseley)
Trends we’ll be looking at:
Atomic Radius
Ionic (Size) Radius
Ionization Energy
3. Electronegativity

21. Atomic (Size) Radius Atomic Radius – size of an atom
(distance from nucleus to outermost e-)

22. Atomic Radius Trend
Group Trend – As you go down a column, atomic radius increases
As you go down, e- are filled into orbitals that are farther away from the nucleus (attraction not as strong)
Periodic Trend – As you go across a period (L to R), atomic radius decreases
As you go L to R, e- are put into the same orbital, but more p+ and e- total (more attraction = smaller size)

23. Ionic Radius
Ionic Radius –
size of an atom when it is an ion

24. Ionic Radius Trend
Metals – lose e-, which means more p+ than e- (more attraction) SO…
Cation Radius < Neutral Atomic Radius
Nonmetals – gain e-, which means more e- than p+ (not as much attraction) SO…
Anion Radius > Neutral Atomic Radius

25. Ionic Radius Trend
Group Trend – As you go down a column, ionic radius increases
Periodic Trend – As you go across a period (L to R), cation radius decreases,
anion radius decreases, too.
As you go L to R, cations have more attraction (smaller size because more p+ than e-). The anions have a larger size than the cations, but also decrease L to R because of less attraction (more e- than p+)

26. Ionic Radius

27. Ionic Radius
How do I remember this????? The more electrons that are lost, the greater the reduction in size. Li+1 Be+2 protons 3 protons 4 electrons 2 electrons 2 Which ion is smaller?

28. Ionic Radius
How do I remember this??? The more electrons that are gained, the greater the increase in size. P-3 S-2 protons 15 protons 16 electrons 18 electrons 18 Which ion is smaller?

29. Ionization Energy
Ionization Energy – energy needed to remove outermost e-

30. Ionization Energy
Group Trend – As you go down a column, ionization energy decreases
As you go down, atomic size is increasing (less attraction), so easier to remove an e-
Periodic Trend – As you go across a period (L to R), ionization energy increases
As you go L to R, atomic size is decreasing (more attraction), so more difficult to remove an e-
(also, metals want to lose e-, but nonmetals do not)

31. Electronegativity
Electronegativity- tendency of an atom to attract e-

32. Electronegativity Trend
Group Trend – As you go down a column, electronegativity decreases
As you go down, atomic size is increasing, so less attraction to its own e- and other atom’s e-
Periodic Trend – As you go across a period (L to R), electronegativity increases
As you go L to R, atomic size is decreasing, so there is more attraction to its own e- and other atom’s e-

33. Reactivity Reactivity – tendency of an atom to react
Metals – lose e- when they react, so metals’ reactivity is based on lowest Ionization Energy (bottom/left corner) Low I.E = High Reactivity
Nonmetals – gain e- when they react, so nonmetals’ reactivity is based on high electronegativity (upper/right corner)
High electronegativity = High reactivity

34. Metallic Character Properties of a Metal – 1. Easy to shape
Conduct electricity 3. Shiny
Group Trend – As you go down a column, metallic character increases
Periodic Trend – As you go across a period (L to R), metallic character decreases (L to R, you are going from metals to non-metals

35. Exothermic Reactions
An exothermic reaction is a chemical reaction that releases energy in the form of light, heat, or sound.

36. Endothermic RXN
An endothermic reaction is a chemical reaction in which energy (heat, light, etc.) is absorbed.

38. Chemistry of Living Systems
Which element contains four valence electrons:
Sodium
Chlorine
Carbon
Neon 1 7 4 8
# valence
electrons
Carbon

39. Chemistry of Living Systems
An organic molecule contains the element:
Oxygen
Hydrogen
Carbon
Iron

40. Chemistry of Living Systems
3. The molecule shown is an
alcohol
organic acid
sugar
ester
Ethanol C H OH OH
(Hydroxyl group)

41. Chemistry of Living Systems
4. The molecule shown is an
alcohol
organic acid
sugar
ester C H OH O
COOH
(Carboxyl group)

42. Chemistry of Living Systems
8. The molecule shown is an
amino acid
sugar
alcohol
lipid H H O H C C C OH
COOH
(Carboxyl group)
NH2 H
NH2
(Amine group)

43. Chemistry of Living Systems
5. Which compound contains Carbon?
lipid
carbohydrate
protein
Nucleic acid
all of the above

44. Chemistry of Living Systems
6. Which compound contains Carbon, Hydrogen and Oxygen?
lipid
carbohydrate
protein
Nucleic acid
all of the above

45. Organic Polymer Elements
Carbohydrates C, H, O
Lipids C, H, O
Proteins C, H, O, N, & sometimes S
Nucleic Acid C, H, O, N, P

46. Enthalpy is a measure of the total energy of a thermodynamic system
Enthalpy is a measure of the total energy of a thermodynamic system. It includes the system's
internal energy and thermodynamic potential (a state function), as well as its volume and
pressure (the energy required to "make room for it" by displacing its environment, which is
an extensive quantity). The unit of measurement for enthalpy in the (SI) is the joule, but
other historical, conventional units are still in use, such as the British thermal unit and the calorie.