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
Describe and explain the observed trends in atomic size, ionization energy, Proceeding down the groups of the periodic table, we find that cations of
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
These periodic trends can clearly be seen in atomic radii, ionic radii, ionization energies and electronegativities These specific trends will be investigated
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
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
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):
tions about atomic size, electronegativity, ionization energies, bonding, solubility, and reactivity In this activity you will look at a few periodic
tDescribe and explain the observed trends in atomic -size, ionization energy, and electron affinity of
the elementsThe 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
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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
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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
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ps oγγαwpπγsr γé γvs β°ozz βwWs ét γvs_H 7 βvszz oâr γvs αsβπzγwâu zoαus szsqγαéâtszsqγαéâ αsøπzβwéâβ3 Qéα s'o°øzs1
qvzéαwâs1 -wγv oâ PL σozπs ét t89C yU4°éz1 voβ γvs vwuvsβγ σozπs ét oâV szs°sâγ wâ γvs øsαwérwq γopzs3 evs PL ét
tzπéαwâs wβ t877 yU4°éz3 hvsâ -s orr oâ szsqγαéâ γé o tzπéαwâs oγé° γé téα° o tzπéαwrs oâwéâ -Q
t.1 -s orr oâ szsqγαéâγé γvs_H 7 βvszz3 evs szsqγαéâ wβ oγγαoqγsr γé γvs âπqzsπβ1 pπγ γvsαs wβ ozβé βwuâwtwqoâγ αsøπzβwéâ tαé° γvs éγvsα
szsqγαéâβ ozαsorV øαsβsâγ wâ γvwβ β°ozz σozsâqs βvszz3 evs qvzéαwâs oγé° voβ γvs βo°s szsqγαéâ qéâtwuπαoγwéâ wâ γvs
σozsâqs βvszz1 pπγ psqoπβs γvs sâγsαwâu szsqγαéâ wβ uéwâu wâγé γvs_H 8 βvszz1 wγ éqqπøwsβ o qéâβwrsαopzV zoαusα αsuwéâ ét
βøoqs oâr γvs szsqγαéâtszsqγαéâ αsøπzβwéâβ oαs αsrπqsr3 evs sâγsαwâu szsqγαéâ résβ âéγ s'øsαwsâqs oβ °πqv αsøπzβwéâ
oâr γvs qvzéαwâs oγé° oqqsøγβ oâ orrwγwéâoz szsqγαé2â °éαs αsorwzV3332Chapter 6 Electronic Structure and Periodic Propert-ies of Elements3DEO?KJPAJPEO=R=EH=>HABKNBNAA=PDPPL/content/col11760/1.9
Inlyvj 7/47Sghr udqrhnm ne sgd odqhnchb s_akd chrok_xr sgd -dkdbsqnm _eehmhsx u_ktdr (hm jI/lnk) enq rdkdbsd-c dkdldmsr.
fwt ħΦéħtΦαxtΨ sxΨrβΨΨts xè αwxΨ Ψtrαxéè /Ψxπt éu pαéµΨ pès xéèΨ3 tuutrαxγt èβr°tpΦ rwpΦvt3 xéèxπpαxéè tètΦvxtΨ3 pès
t°trαΦéè puuxèxαxtΨ0 pΦt rtèαΦp° αé βèstΦΨαpèsxèv rwtµxrp° Φtprαxγxαν5 SéΦ tλpµħ°t3 qtrpβΨt u°βéΦxèt wpΨ pè tètΦvtαxrp°°ν
upγéΦpq°t RN pès p °pΦvt tètΦvν qpΦΦxtΦ αé xéèxπpαxéè /VR03 xα xΨ µβrw tpΨxtΦ αé uéΦµ u°βéΦxèt pèxéèΨ αwpè rpαxéèΨ5
[tαp°°xr ħΦéħtΦαxtΨ xèr°βsxèv réèsβrαxγxαν pès µp°°tpqx°xαν /αwt pqx°xαν αé qt uéΦµts xèαé ΨwttαΨ0 stħtès éè wpγxèv
t°trαΦéèΨ αwpα rpè qt Φtµéγts tpΨx°ν5 fwβΨ3 µtαp°°xr rwpΦprαtΦ xèrΦtpΨtΨ pΨ θt µéγt séθè p vΦéβħ pès strΦtpΨtΨ
prΦéΨΨ p ħtΦxés xè αwt Ψpµt αΦtès éqΨtΦγts uéΦ pαéµxr Ψxπt qtrpβΨt xα xΨ tpΨxtΦ αé Φtµéγt pè t°trαΦéè αwpα xΨ upΦαwtΦ
pθpν uΦéµ αwt èβr°tβΨ5Bg_osdq 6 Dkdbsqnmhb Rsqtbstqd _mc Odqhnchb Oqnodqs-hdr ne Dkdldmsr333
R°trαΦéè réèuxvβΦpαxéèΨ p°°éθ βΨ αé βèstΦΨαpès µpèν ħtΦxésxr αΦtèsΨ5 Péγp°tèα ΦpsxβΨ xèrΦtpΨtΨ pΨ θt µéγt séθè p
vΦéβħ qtrpβΨt αwt_°tγt° /éΦqxαp° Ψxπt0 xèrΦtpΨtΨ5 Péγp°tèα ΦpsxβΨ µéΨα°ν strΦtpΨtΨ pΨ θt µéγt °tuα αé Φxvwα prΦéΨΨ
p ħtΦxés qtrpβΨt αwt tuutrαxγt èβr°tpΦ rwpΦvt tλħtΦxtèrts qν αwt t°trαΦéèΨ xèrΦtpΨtΨ3 pès αwt t°trαΦéèΨ pΦt ħβ°°ts
xè αxvwαtΦ αé αwt èβr°tβΨ5 Nèxéèxr Φpsxx pΦt °pΦvtΦ αwpè αwt ħpΦtèα pαéµ3 θwx°t rpαxéèxr Φpsxx pΦt Ψµp°°tΦ3 qtrpβΨt αwt
èβµqtΦ éu γp°tèrt t°trαΦéèΨ wpΨ rwpèvts θwx°t αwt èβr°tpΦ rwpΦvt wpΨ Φtµpxèts réèΨαpèα5 Véèxπpαxéè tètΦvν /αwt
tètΦvν pΨΨérxpαts θxαw uéΦµxèv p rpαxéè0 strΦtpΨtΨ séθè p vΦéβħ pès µéΨα°ν xèrΦtpΨtΨ prΦéΨΨ p ħtΦxés qtrpβΨt xα
xΨ tpΨxtΦ αé Φtµéγt pè t°trαΦéè uΦéµ p °pΦvtΦ3 wxvwtΦ tètΦvν éΦqxαp°5 R°trαΦéè puuxèxαν /αwt tètΦvν pΨΨérxpαts θxαw
uéΦµxèv pè pèxéè0 xΨ µéΦt upγéΦpq°t /tλéαwtΦµxr0 θwtè t°trαΦéèΨ pΦt ħ°prts xèαé °éθtΦ tètΦvν éΦqxαp°Ψ3 r°éΨtΦ αé αwt
èβr°tβΨ5 fwtΦtuéΦt3 t°trαΦéè puuxèxαν qtréµtΨ xèrΦtpΨxèv°ν ètvpαxγt pΨ θt µéγt °tuα αé Φxvwα prΦéΨΨ αwt ħtΦxésxr αpq°t
pès strΦtpΨtΨ pΨ θt µéγt séθè p vΦéβħ5 SéΦ qéαw VR pès t°trαΦéè puuxèxαν spαp3 αwtΦt pΦt tλrtħαxéèΨ αé αwt αΦtèsΨ
θwtè stp°xèv θxαw réµħ°tαt°ν ux°°ts éΦ wp°u4ux°°ts 4ΨβqΨwt°°Ψ5
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.