trends in the periodic table:
DESCRIPTION
Trends in the periodic table:. Ionization Energy Atomic Radius Electron Affinity Electronegativity. Background. Electrons can jump between shells (Bohr’s model supported by line spectra) The electrons can be pushed so far that they escape the attraction of the nucleus - PowerPoint PPT PresentationTRANSCRIPT
Trends in the periodic Trends in the periodic table:table:
Ionization EnergyIonization EnergyAtomic RadiusAtomic Radius
Electron AffinityElectron AffinityElectronegativityElectronegativity
BackgroundBackground• Electrons can jump between shells (Bohr’s
model supported by line spectra)• The electrons can be pushed so far that they
escape the attraction of the nucleus• Losing an electron is called ionization• An ion is an atom that has either a net
positive or net negative charge• Q: what would the charge be on an atom
that lost an electron? Gained two electrons?• A: +1 (because your losing a -ve electron)• A: -2 (because you gain 2 -ve electrons)
Ionization energyIonization energy• Ionization energy is the energy required to
remove one outer electron from an atom• We will be examining the trends in ionization
energy in groups and periods• Handout• Note: atomic radius is the distance from the
nucleus to the outer electron shell• Follow directions on sheet and answer
questions (you can use textbook for help)• Ignore H when looking at trends, look at many
periods/groups when summarizing trends
Periodic table Periodic table
trendstrends Answers Answers
Ionization energy vs. atomic numberIonization energy vs. atomic number
Ca
K
H
He
Li
B
Be C
N O
F
Ne
Na
MgAl
SiP S
Cl
Ar
0
500
1000
1500
2000
2500
0 2 4 6 8 10 12 14 16 18 20
Element
Ioni
zatio
n en
ergy
(kJ
/mol
)
Atomic radius vs. atomic numberAtomic radius vs. atomic number
Ca
K
H He
Li
B
Be
C N O FNe
NaMg
Al Si P S Cl
Ar
0
50
100
150
200
250
0 2 4 6 8 10 12 14 16 18 20
Element
Ato
mic
Rad
ius
(pm
)
AnswersAnswers2 a) – He, Ne, Ar, Noble gases2 b) – Li, Na, K, Alkali metals3 a) – Li, Na, K, Alkali metals3 b) – He, Ne, Ar, Noble gases4. As one increases, the other decreases5. Ionization energy increases
Atomic radius decreases6. Ionization energy decreases
Atomic radius increases
7.
11p+ 12n°
Na has 11 electrons
Na+ has 10 electrons
Ne has 10 electrons
11p+ 12n°
10p+ 10n°
electron configuration of Na+ resembles NeAlkali metals become like noble gases8. Radius increases because shells are added
Increased radius will make it easier to lose an electron because of greater distance between positive and negative charges
9.Proton # increases. More protons means greater attraction between nucleus and outer electron thus higher ionization energy.The greater attraction also means that outer electrons are brought closer to the nucleus, thus smaller atomic radius results.
Li (enc = 1)
+++
Be (enc = 2)
++++
B (enc = 3)
+++++
10.Noble gases are ignored11.Electron affinity is energy associated with an
atom gaining an electron. It is highest in the top right where atoms are smallest with the greatest number of protons
12.Electronegativity is a number that describes the relative ability of an atom (when bonded) to attract electrons. The trend is the same as affinity for the same reason
AnswersAnswers2 a) – He, Ne, Ar (1), Noble gases (1)2 b) – Li, Na, K (1), Alkali metals (1)3 a) – Li, Na, K, Alkali metals (1)3 b) – He, Ne, Ar, Noble gases (1)4. As one increases, the other decreases (1)5. Ionization energy increases (1)
Atomic radius decreases (1)6. Ionization energy decreases (1)
Atomic radius increases (1)
7.
11p+ 12n°
Na has 11 electrons
Na+ has 10 electrons
Ne has 10 electrons
11p+ 12n°
10p+ 10n°
Diagram of Na(1) & Na+(1), Na+ resembles Ne (1)Alkali metals become like noble gases (1)8. Radius increases because shells are added (1)
Increased radius will make it easier to lose an electron because of greater distance between positive and negative charges (1)
9.Proton # increases (1). More protons means greater attraction between nucleus and outer electron (1) thus higher ionization energy.The greater attraction also means that outer electrons are brought closer to the nucleus, thus smaller atomic radius results.
Li (enc = 1)
+++
Be (enc = 2)
++++
B (enc = 3)
+++++
10.Noble gases are ignored (1)11.Electron affinity is energy associated with an atom
gaining an electron (1). It is highest in the top right (1) where atoms are smallest with the greatest number of protons
12.Electronegativity is a number that describes the relative ability of an atom (when bonded) to attract electrons (1). The trend is the same as affinity (1) for the same reason Total: /24
Note: graphs from day 1 were marked separately
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