Ch.8 - Periodic Properties of the ElementsWorksheetSee all chapters
All Chapters
Ch.1 - Intro to General Chemistry
Ch.2 - Atoms & Elements
Ch.3 - Chemical Reactions
BONUS: Lab Techniques and Procedures
BONUS: Mathematical Operations and Functions
Ch.4 - Chemical Quantities & Aqueous Reactions
Ch.5 - Gases
Ch.6 - Thermochemistry
Ch.7 - Quantum Mechanics
Ch.8 - Periodic Properties of the Elements
Ch.9 - Bonding & Molecular Structure
Ch.10 - Molecular Shapes & Valence Bond Theory
Ch.11 - Liquids, Solids & Intermolecular Forces
Ch.12 - Solutions
Ch.13 - Chemical Kinetics
Ch.14 - Chemical Equilibrium
Ch.15 - Acid and Base Equilibrium
Ch.16 - Aqueous Equilibrium
Ch. 17 - Chemical Thermodynamics
Ch.18 - Electrochemistry
Ch.19 - Nuclear Chemistry
Ch.20 - Organic Chemistry
Ch.22 - Chemistry of the Nonmetals
Ch.23 - Transition Metals and Coordination Compounds

Solution: Place the following in order of increasing  IEI.N     F     Asa. As < F < Nb. F < As < Nc. As < N < Fd. F < N < Ase. N < As < F


Place the following in order of increasing  IEI.

N     F     As

a. As < F < N

b. F < As < N

c. As < N < F

d. F < N < As

e. N < As < F


We are asked to arrange the following in increasing EIor the first ionization energy. 

Ionization energy (I. E.) is the energy required to remove an electron from a gaseous atom or ion.

First I.E. corresponds to removing the first valence electron from a neutral atom

Second I.E. refers to removing a second electron

Third I.E. refers to removing the third electron

The trend of the ionization energies of the elements can be observed in the periodic table:

increases going from left to right of a period

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