[PDF] 65 Periodic Variations in Element Properties




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[PDF] Mastering Periodic Trends

Atomic radius is the distance from the atom's nucleus to the outer edge of the electron cloud In general, atomic radius decreases across a period and increases 

[PDF] 65 Periodic Variations in Element Properties

Describe and explain the observed trends in atomic size, ionization energy, Proceeding down the groups of the periodic table, we find that cations of 

[PDF] ATOMIC SIZE

In this periodic table, the relative sizes (not absolute - there are no measurements) are shown The sizes of the noble gas atoms (gray) can't really be 

[PDF] PERIODIC TRENDS The periodic table is arranged in order of

These periodic trends can clearly be seen in atomic radii, ionic radii, ionization energies and electronegativities These specific trends will be investigated 

[PDF] Element Entry Identification What is the Atomic Number? Terms

Check the Periodic Table to find out how many electrons each element actually has The atomic radius is a measure of the size of an atom The larger the

[PDF] Periodic Table Trends - Wiggins School District

Write a letter to your friend explaining atomic radii, ionization energy and electronegativity Include an explanation of the trends for each as you move across 

[PDF] Chem 1010/1800 Tip Sheet - Periodic Trends - Ontario Tech University

Atomic radius: a measure of an atom's size, using the distance from the centre of the nucleus to the outermost electron shell Effective nuclear charge (Zeff): 

[PDF] Can the properties of an element be predicted using a periodic table?

tions about atomic size, electronegativity, ionization energies, bonding, solubility, and reactivity In this activity you will look at a few periodic 

[PDF] 65 Periodic Variations in Element Properties 138072_7PeriodicVariationsinElementProperties.pdf

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By the end of this section, you will be able- to:

tDescribe and explain the observed trends in atomic -size, ionization energy, and electron affinity of

the elements

The elements in groups (vertical columns) of the periodic table exhibit similar chemical behavior. This similarity

occurs because the members of a group have the same number and distribution of electrons in their valence shells.

However, there are also other patterns in chemical properties on the periodic table. For example, as we move down

a group, the metallic character of the atoms increases. Oxygen, at the top of group 16 (6A), is a colorless gas; in the<;=OvoéΨsΠ B QzsqΨΠèµwq dΨΠαqΨαΠs oµr asΠwèrwq aΠèésΠΨ4wsΦ èt Qzs°sµΨΦ3DEO?KJPAJPEO=R=EH=>HABKNBNAA=PDPPL6qèµΨsµΨ6qèz::CB86:5Emiddle of the group, selenium is a semiconducting solid; and, toward the bottom, polonium is a silver-grey solid thatconducts electricity.

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varyperiodicallyastheelectronicstructureoftheelementschanges.Theyare(1)size(radius)ofatomsandions,(2)

ionization energies, and (3) electron affinities.

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The amount of energy required to remove the most loosely bound electron from a gaseous atom in its ground state is

called its firstjpoj°bujpo fofshz(IE1). The first ionization energy for an element, X, is the energy required to form a

cation with +1 charge: ڮ 2). ڮ

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The values of first ionization energy for the elements are given inInlyvj 7/46. Within a period, the IE1generally

increases with increasingM. Down a group, the IE1value generally decreases with increasingM. There are some

systematic deviations from this trend, however. Note that the ionization energy of boron (atomic number 5) is less

than that of beryllium (atomic number 4) even though the nuclear charge of boron is greater by one proton. This can be

explained because the energy of the subshells increases as[increases, due to penetration and shielding (as discussed

previously in this chapter). Within any one shell, theeelectrons are lower in energy than thebelectrons. This means

that aneelectron is harder to remove from an atom than abelectron in the same shell. The electron removed during

the ionization of beryllium ([He]2e2) is aneelectron, whereas the electron removed during the ionization of boron

([He]2e22b1) is abelectron; this results in a lower first ionization energy for boron, even though its nuclear charge

is greater by one proton. Thus, we see a small deviation from the predicted trend occurring each time a new subshell

begins.Chapter 6 Electronic Structure and Periodic Propert-ies of Elements329

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20)OpΨts éè αwtxΦ ħéΨxαxéèΨ xè αwt ħtΦxésxr αpq°t3 4°xΨα αwt ué°°éθxèv pαéµΨ xè éΦstΦ éu xèrΦtpΨxèv 4ΦpsxβΨF [v3 Pp3 dq3

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22)OpΨts éè αwtxΦ ħéΨxαxéèΨ xè αwt ħtΦxésxr αpq°t3 4°xΨα αwt ué°°éθxèv xéèΨ xè éΦstΦ éu xèrΦtpΨxèv Φ4psxβΨF X23 Pp;23

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79.Which atom and/or ion is (are) isoelectronic w-ith Br+: Se2+, Se, As-, Kr, Ga3+, Cl-?

80.Which of the following atoms and ions is (are)- isoelectronic with S2+: Si4+, Cl3+, Ar, As3+, Si, Al3+?

81.Compare both the numbers of protons and electrons -present in each to rank the following ions in -order of

increasing radius: As

3-, Br-, K+, Mg2+.

82.Of the five elements Al, Cl, I, Na, Rb, -which has the most exothermic reaction? (E repr-esents an atom.) What

name is given to the energy for the reaction? Hint: note the process -depicted doesnotcorrespond to electron affinity

Чڮ name is given to the energy for the reaction? ڮ different sizes even though they contain the same n-umber of electrons.

85.Which main group atom would be expected to have -the lowest second ionization energy?

86.Explain why Al is a member of group 13 -rather than group 3?344Chapter 6 Electronic Structure and Periodic Propert-ies of Elements3DEO?KJPAJPEO=R=EH=>HABKNBNAA=PDPPL/content/col11760/1.9


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