5.2 Electron Configuration & The Periodic Table Chapter 5 The Periodic Law 5.2 Electron Configuration & The Periodic Table

In the modern periodic table, elements are arranged in order of increasing atomic number.

METALS METALLOIDS NONMETALS In the periodic table below, indicate the location of the groups, periods, alkali metals, alkaline earth metals, halogens, noble gases, lanthanides, actinides, transition metals, inner transition metals, main group elements, metals, nonmetals and metalloids. METALS METALLOIDS NONMETALS

80% of elements are metals. Most solids (Hg is liquid) Luster – shiny. Ductile – drawn into thin wires. Malleable – hammered into sheets. Conductors of heat and electricity. Include transition metals – “bridge” between elements on left & right of table 80% of elements are metals.

Uses of Iron, Copper, and Aluminum The metals iron, copper, and aluminum have many important uses. How each metal is used is determined by its properties.

Nonmetals Properties are generally opposite of metals Poor conductors of heat and electricity Low boiling points Most are gases at room temperature Few are brittle solids (break easily), phosphorus and sulfur One, bromine, is a dark red liquid Chemical properties vary

Metalloids stair-step pattern 6 elements Have properties similar to metals and non-metals Ability to conduct heat and electricity varies with temp Better than non-metals but not metals *The behavior of a metalloid can be controlled by changing conditions.

Uses of Metalloids If a small amount of boron is mixed with silicon, the mixture is a good conductor of electric current. Silicon can be cut into wafers, and used to make computer chips.

Let’s Compare! Metals Nonmetals Metalloids Good conductors of heat and electricity Malleable Ductile Luster Typically solids at room temperature Solids, liquids and gases at room temperature Solids are brittle and dull Poor conductors of heat and electricity Have properties of both metals and nonmetals Mostly brittle solids Intermediate conductors of electricity- AKA semiconductors

Sublevel Blocks on the Periodic Table 1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18 Sublevel Blocks on the Periodic Table

PERIODS

GROUPS

In the periodic table below, indicate the location of the groups, periods, alkali metals, alkaline earth metals, halogens, noble gases, lanthanides, actinides, transition metals, inner transition metals, main group elements, metals, nonmetals and metalloids. MAIN GROUP ELEMENTS

s-Block Elements: Group 1 s1 - ALKALI METALS

1s1 1s22s1 1s22s22p63s1 1s22s22p63s23p64s1 1s22s22p63s23p64s23d104p65s1 1s22s22p63s23p64s23d104p65s24d10 5p66s1 1s22s22p63s23p64s23d104p65s24d105p66s24f145d106p67s1 H 1 Li 3 Na 11 K 19 Rb 37 Cs 55 Fr 87 Do you notice any similarity in these configurations of the alkali metals?

s-Block Elements: Group 2 s2 - ALKALINE-EARTH METALS

d-Block Elements: Groups 3-18 TRANSITION METALS (Level – 1) d1 d2 d3 d4 d5 d6 d7 d8 d9 d10

p-Block Elements: Group 17 HALOGENS – p5

p-Block Elements: Group 18 NOBLE GASES – p6

1s2 1s22s22p6 1s22s22p63s23p6 1s22s22p63s23p64s23d104p6 1s22s22p63s23p64s23d104p65s24d105p6 1s22s22p63s23p64s23d104p65s24d10 5p66s24f145d106p6 He Do you notice any similarity in the configurations of the noble gases? 2 Ne 10 Ar 18 Kr 36 Xe 54 Rn 86

f-Block Elements: Lanthanides and Actinides INNER TRANSITION (Rare Earth) METALS f1 f2 f3 f4 f5 f6 f7 f8 f9 f10 f11 f12 f13 f14

f-Block Elements: Lanthanides and Actinides 4f1 - 4f14

f-Block Elements: Lanthanides and Actinides 5f1 - 5f14

Elements in the s - blocks Alkali metals end in s1 Alkaline earth metals end in s2 should include He, but… He has properties of noble gases has a full outer level of e-’s group 8A.

Transition Metals - d block Note the change in configuration. s1 d5 s1 d10 d1 d2 d3 d5 d6 d7 d8 d10

The P-block p1 p2 p3 p4 p6 p5

F - block f1 f5 f2 f3 f4 f6 f7 f8 f9 f10 f11 f12 f14 f13 Called “inner transition elements” f1 f5 f2 f3 f4 f6 f7 f8 f9 f10 f11 f12 f14 f13

Each period # = energy level for s & p orbitals. 1 2 3 4 5 6 7 Period Number Each period # = energy level for s & p orbitals.

3d 4d 5d “d” orbitals fill up in levels 1 less than period # first d is 3d found in period 4. 1 2 3 4 5 6 7 3d 4d 5d

f orbitals start filling at 4f….2 less than period # 1 2 3 4 5 6 7 4f 5f f orbitals start filling at 4f….2 less than period #

Electron Configurations in Groups 6.2 Electron Configurations in Groups The Noble Gases The noble gases are the elements in Group 8A of the periodic table. The electron configurations for the first four noble gases in Group 8A are listed below.

Electron Configurations in Groups 6.2 Electron Configurations in Groups In atoms of the Group 1A elements below, there is only one electron in the highest occupied energy level.

Electron Configurations in Groups 6.2 Electron Configurations in Groups In atoms of the Group 4A elements below, there are four electrons in the highest occupied energy level.

Transition Elements Blocks of Elements 6.2 This diagram classifies elements into blocks according to sublevels that are filled or filling with electrons. Interpreting Diagrams In the highest occupied energy level of a halogen atom, how many electrons are in the p sublevel?

Properties of Alkali Metals Extremely reactive Readily react with water and air Silvery in appearance Soft enough to cut with a knife Lower densities than other metals Lower melting points than other metals

Properties of Alkaline-Earth Metals Harder & stronger than alkali metals Higher densities & melting points than alkali metals Less reactive than alkali metals

Properties of Halogens Most reactive nonmetals React readily with most metals to form salts Most electronegative elements

Properties of Noble Gases Least reactive elements highest occupied energy levels completely filled with octet of electrons (except He, which only requires 2 electrons to be filled).

Properties of Transition Metals High densities High melting points Good conductors of heat & electricity High luster Less reactive than alkali and alkaline-earth metals

Properties of p Block Metals Harder and more dense than the s block metals Softer and less dense than the d block metals.

Properties of Lanthanides Soft, silvery metals Similar reactivity to alkaline-earth metals

Properties of Actinides All radioactive The first 4 have been found naturally on Earth

The Properties of Group 1: the Alkali Metals Easily lose 1 valence electron (Reducing agents) React violently with water React with halogens to form salts

The Properties of Group 1: the Alkali Earth Metals Easily loses 2 valence electron (Reducing agents) Harder, denser, stronger than Group 1 metals Higher melting points Less reactive than Group 1, but too reactive to be found free in nature