periodic relationships among the elements chapter 7 copyright © the mcgraw-hill companies, inc....

Periodic Relationships Among the Elements

Chapter 7

Copyright © The McGraw-Hill Companies, Inc.  Permission required for reproduction or display.

8.1

When the Elements Were Discovered

8.3

Atomic radius – one-half the distance between the two nuclei in two adjacent metal atoms or in a diatomic molecule

8.3

General Trend in First Ionization Energies

8.4

Increasing First Ionization Energy

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Electron affinity is the negative energy change that occurs when an electron is accepted by an atom in the gaseous state to form an anion.

X (g) + e- X-(g)

8.5

F (g) + e- F-(g)

O (g) + e- O-(g)

H = -328 kJ/mol EA = +328 kJ/mol

H = -141 kJ/mol EA = +141 kJ/mol

Electron affinity – the energy change in kJ accompanying the addition of 1 mol of e- to 1 mol of gaseous atoms or ions.

SAMPLE PROBLEM Ranking Elements by Atomic Size

PLAN:

SOLUTION:

PROBLEM: Using only the periodic table (not Figure 8.15)m rank each set of main group elements in order of decreasing atomic size:

(a) Ca, Mg, Sr (b) K, Ga, Ca (c) Br, Rb, Kr (d) Sr, Ca, Rb

Elements in the same group increase in size and you go down; elements decrease in size as you go across a period.

(a) Sr > Ca > Mg These elements are in Group 2A(2).

(b) K > Ca > Ga These elements are in Period 4.

(c) Rb > Br > Kr Rb has a higher energy level and is far to the left. Br is to the left of Kr.

(d) Rb > Sr > Ca Ca is one energy level smaller than Rb and Sr. Rb is to the left of Sr.

SAMPLE PROBLEM Ranking Elements by First Ionization Energy

PLAN:

SOLUTION:

PROBLEM: Using the periodic table only, rank the elements in each of the following sets in order of decreasing IE1:

(a) Kr, He, Ar (b) Sb, Te, Sn (c) K, Ca, Rb (d) I, Xe, Cs

IE decreases as you proceed down in a group; IE increases as you go across a period.

(a) He > Ar > Kr

(b) Te > Sb > Sn

(c) Ca > K > Rb

(d) Xe > I > Cs

Group 8A(18) - IE decreases down a group.

Period 5 elements - IE increases across a period.

Ca is to the right of K; Rb is below K.

I is to the left of Xe; Cs is furtther to the left and down one period.

Group 1A Elements (ns1, n 2)

8.6

Group 1A Elements

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8.6

Low Ionization energies. Tendency to lose the single valance electron They are very reactive, never found in nature in pure state

Group 2A Elements (ns2, n 2)

8.6

Group 2A Elements

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8.6

Alkaline earth metals Metallic character increases from top to bottom

Group 3A Elements (ns2np1, n 2)

8.6

Group 3A Elements

8.6

Boron is a metalloid; the rest are metals

Group 4A Elements (ns2np2, n 2)

8.6

Group 4A Elements

8.6

Carbon a non metalSilicon and Germanium are metalloidsThen all metals

Group 5A Elements

8.6

Group 5A Elements

8.6

Nitrogen and Phosphorous are non metalsArsenic and antimony are metalloidsBismuth is a metal

Group 6A Elements

8.6

Group 6A Elements

8.6

The 1st three are non metalsThe last two are metalloids

Group 7A Elements

8.6

Group 7A Elements

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8.6

All are halogens and are non metalsGreat reactivityNever found in their element form in natureHigh ionization energies Large positive electron affinity

Group 8A Elements

8.6

Completely filled ns and np subshells. Highest ionization energy of all elements.No tendency to accept extra electrons.

Trends in metallic behavior.