chapter 6.3
DESCRIPTION
TRANSCRIPT
![Page 1: Chapter 6.3](https://reader033.vdocuments.mx/reader033/viewer/2022061119/546a6fb4af7959973b8b61ee/html5/thumbnails/1.jpg)
Chapter 6:The Periodic Table
Section 3:Periodic Trends
![Page 2: Chapter 6.3](https://reader033.vdocuments.mx/reader033/viewer/2022061119/546a6fb4af7959973b8b61ee/html5/thumbnails/2.jpg)
Describe trends among elements for shielding of nuclear charge;
Describe trends among elements for atomic size;
Explain how ions form; Define ionization energy; Describe trends among elements for ionization
energy and ionic radius; Define electronegativity; and Describe trends among elements for
electronegativity
Students will be able to…
![Page 3: Chapter 6.3](https://reader033.vdocuments.mx/reader033/viewer/2022061119/546a6fb4af7959973b8b61ee/html5/thumbnails/3.jpg)
Electrons (e-) are attracted to protons (p+) Trends relate to how those added protons
and electrons interact As you add 2nd p+ and e-, not much between
them Adding e- to 2nd energy level, have inner e-
shielding charge of added p+
As you move across the table, added e-
experience same level of shielding
The trend behind the trends...
![Page 4: Chapter 6.3](https://reader033.vdocuments.mx/reader033/viewer/2022061119/546a6fb4af7959973b8b61ee/html5/thumbnails/4.jpg)
Nuclear charge and shielding
Nuclear Charge
Shielding
Increases (adding protons)
Constant ( e- get same view of nucleus)
Incre
ase
s (ad
din
g p
roto
ns
Incre
ase
s (more
le
vels)
![Page 5: Chapter 6.3](https://reader033.vdocuments.mx/reader033/viewer/2022061119/546a6fb4af7959973b8b61ee/html5/thumbnails/5.jpg)
Atomic radius: half of distance between nuclei of two atoms of the same element when the atoms are joined
General trend: Increases down a group Decreases across a period
Trends in Atomic Size
![Page 6: Chapter 6.3](https://reader033.vdocuments.mx/reader033/viewer/2022061119/546a6fb4af7959973b8b61ee/html5/thumbnails/6.jpg)
Trends in Atomic Size
![Page 7: Chapter 6.3](https://reader033.vdocuments.mx/reader033/viewer/2022061119/546a6fb4af7959973b8b61ee/html5/thumbnails/7.jpg)
Atomic Radius From Shielding
Atomic Radius
Decreases (shielding constant, so p+suck in e-)
Incre
ase
s (levels w
in)
![Page 8: Chapter 6.3](https://reader033.vdocuments.mx/reader033/viewer/2022061119/546a6fb4af7959973b8b61ee/html5/thumbnails/8.jpg)
Ion: atom or group of atoms that has a charge
Cation: Ion with a positive charge
You’ll get a charge out of this...
![Page 9: Chapter 6.3](https://reader033.vdocuments.mx/reader033/viewer/2022061119/546a6fb4af7959973b8b61ee/html5/thumbnails/9.jpg)
Ion: atom or group of atoms that has a charge
Cation: Ion with a positive charge Anion: ion with a negative charge
You’ll get a charge out of this...
![Page 10: Chapter 6.3](https://reader033.vdocuments.mx/reader033/viewer/2022061119/546a6fb4af7959973b8b61ee/html5/thumbnails/10.jpg)
Cations always smaller than neutral atom◦ Lose one e-◦ More protons, suck in remaining
electrons Anions always bigger than
neutral atom◦ One extra e-
◦ Not as much positive charge to go around
How big is that ion?
![Page 11: Chapter 6.3](https://reader033.vdocuments.mx/reader033/viewer/2022061119/546a6fb4af7959973b8b61ee/html5/thumbnails/11.jpg)
Ionization energy: energy required to remove an electron from an atom in its gaseous state
Generally increases across periods ◦ Shielding constant ◦ Increased nuclear charge holds onto electrons ◦ As get closer to nonmetals, rather gain than lose
Generally decreases down groups ◦ Valence electrons further from nucleus ◦ Easier to pull off
Don’t even think about taking my e-
![Page 12: Chapter 6.3](https://reader033.vdocuments.mx/reader033/viewer/2022061119/546a6fb4af7959973b8b61ee/html5/thumbnails/12.jpg)
Don’t even think about taking my e-
![Page 13: Chapter 6.3](https://reader033.vdocuments.mx/reader033/viewer/2022061119/546a6fb4af7959973b8b61ee/html5/thumbnails/13.jpg)
Ionization Energy
Ionization Energy
Increases (shielding constant, p+hold onto e-)
Decre
ases (fu
rther
aw
ay, e
asie
r to
lose)
![Page 14: Chapter 6.3](https://reader033.vdocuments.mx/reader033/viewer/2022061119/546a6fb4af7959973b8b61ee/html5/thumbnails/14.jpg)
Electronegativity: ability of an atom to attract electrons when in a compound
Cs least electronegative element◦ Lowest ionization energy◦ Loses electrons easily, doesn’t attract them
•F most electronegative element
The flipside of ionization energy
![Page 15: Chapter 6.3](https://reader033.vdocuments.mx/reader033/viewer/2022061119/546a6fb4af7959973b8b61ee/html5/thumbnails/15.jpg)
Electronegativity
Electro-negativit
y
Increases (extra protons pull on electrons)
Decre
ases
(Sh
ield
ing
blo
cks
pu
ll)
![Page 16: Chapter 6.3](https://reader033.vdocuments.mx/reader033/viewer/2022061119/546a6fb4af7959973b8b61ee/html5/thumbnails/16.jpg)
Summary of trendsElectronegativity
Ionization Energy
Increases
Increases
Decrease
Increases
Constant
Decre
ases
Decre
ases
incre
ases
Incre
ases
Incre
ases
Atomic Radius
Nuclear Charge
Shielding
![Page 17: Chapter 6.3](https://reader033.vdocuments.mx/reader033/viewer/2022061119/546a6fb4af7959973b8b61ee/html5/thumbnails/17.jpg)
Describe trends among elements for shielding of nuclear charge?
Describe trends among elements for atomic size;
Explain how ions form? Define ionization energy? Describe trends among elements for ionization
energy and ionic radius? Define electronegativity? Describe trends among elements for
electronegativity?
Can you…?