Chapter 14 - The Periodic Table Chapter 14 - The Periodic Table and Periodic Lawand Periodic Law

• Objectives:– Identify different key features of the periodic table.

– Explain why elements in a group have similar properties.

– Relate the group and period trends seen in the periodic table to the electron configuration of atoms.

• Why this is important:– The periodic table is one of the most useful reference tools

available in chemistry! Understanding its organization and interpreting its data will aid in understanding chemistry concepts.

www.privatehand.com/flash/elements.html

Development of the Periodic Table• In 2003, there were 118 elements known.• The majority of the elements were discovered between

1735 and 1843.• How do we organize all the different elements in a

meaningful way that will allow us to make predictions about undiscovered elements?

• 1869 Dmitri Mendeleev and Lothar Meyer separately arranged the elements in order of increasing atomic mass and into columns with similar properties.

• Mendeleev is given more credit than Meyer because he published his findings first, and he left spaces for elements that were not yet discovered.

• Some of the elements that he predicted were scandium, gallium, and germanium.– In 1871, Mendeleev noted that arsenic (As) properly belonged underneath

phosphorus (P) and not silicon (Si), which left a missing element underneath Si. He predicted a number of properties for this element. In 1886 Germanium (Ge) was discovered. The properties of Ge matched Mendeleev’s predictions.

http://www.chemistrydaily.com/chemistry/upload/a/a1/Dmendeleev.jpg http://www.chemistryexplained.com/images/chfa_03_img0535.jpg

• Mendeleev’s table was not completely correct.

• Arranging elements by atomic mass caused some elements to be put in the wrong groups so that the properties did not exactly match up.

• 1913 English chemist Henry Moseley arranged elements in order of increasing atomic number.

• Problems with order of elements were solved, and there was a clear repeating pattern of properties of the elements in their groups.

• The PERIODIC LAW states there is a “periodic” repetition of chemical and physical properties of the elements when they are arranged by increasing atomic number.

• Periodic means: happening or reoccurring at regular intervals. (definition from Webster’s Dictionary)

http://www.rsc.org/education/teachers/learnnet/periodictable/scientists/moseley.jpg

The Modern TableThe Modern Table• Boxes are arranged in order of increasing atomic #• Elements are grouped into columns by similar

properties• Scientists keep adding elements that were discovered• The final adjustment was when physicist Glenn

Seaborg had the inner-transition elements pulled below the rest of the periodic table and into 2 separate rows (This occurred in the late 1940s)

http://www.lbl.gov/Science-Articles/Research-Review/Magazine/1994/seaborgium-mag.html

• Horizontal rows are called periods• There are 7 periods1

234567

• Vertical columns are called groups or families.• Elements are placed in columns by similar

properties.– b/c of the similar numbers of valence e- they contain!

1 2

13 14 15 16 17

18

3 4 5 6 7 8 9 10 11 12

The Different Groups of Elements1 – 18 system used by all chemists

A & B system is an older American System

A elements are representative elements

B elements are transition elements1A 2A

3A 4A 5A 6A 7A

8A

3B 4B 5B 6B 7B 8B 8B 8B 1B 2B

Representative or Main Group Representative or Main Group ElementsElements

• Wide range of physical & chemical properties.• The whole range of possible valence electrons (1 to 8)• Also called s and p block elements• Here are some important groups:

• Group 1 (1A) contains the alkali metals (remember to NOT include hydrogen)

• Group 2 (2A) contains the alkaline earth metals

Alkali MetalsAlkali Metals• These metals react w/ water to form alkaline (basic)

solutions.• Highly reactive metals that lose their 1 valence electron

to form 1+ ions.• Soft enough to be cut with a knife.• They are stored in oil to prevent reactions with oxygen

and water in the air.

Alkaline Earth MetalsAlkaline Earth Metals• Most of these metals react with oxygen to form

compounds called oxides (the alchemists called them “earths” because of this) and the oxides react w/ water to form alkaline (basic) solutions.

• Not as reactive (but do react easily) & harder than group 1 metals.

• They lose their 2 valence electrons to form 2+ ions.

• Group 17 (7A) contains the halogens• Group 18 (8A) contains the noble gases

HalogensHalogens• Halogen means “salt formers” b/c they react with metals

to form salts (ionic compounds).• F & Cl are gases at room temp., Br is a liquid but it

evaporates easily, and Iodine is a solid that sublimes easily.

• Astatine is radioactive w/ no known uses.• They are the most reactive nonmetals!• 7 valence e- → share or gain 1 e- and they tend to

form 1- ions.

Noble GasesNoble Gases• Last naturally occurring elements to be discovered b/c

they are colorless & unreactive.• Very stable with full valence electrons = 8.

– (except He w/ 2)

• With lots of energy you can get Xe, Kr and Ar compounds. (No known He or Ne compounds)– In 1962 the first compound of the noble gases was prepared:

XeF2, XeF4, and XeF6. (flexible e- arrangments b/c f orbitals)

– To date the only other noble gas compounds known are KrF2 and HArF.

Transition elements (metals)

d-block

f-block

Inner transition elements