periodic properties. atomic size atomic size: the radius of an atom (distance from nucleus to...
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![Page 1: Periodic Properties. Atomic Size Atomic size: the radius of an atom (distance from nucleus to electron cloud) is considered. Measured in angstroms (A)](https://reader035.vdocuments.site/reader035/viewer/2022071807/56649e705503460f94b6d72d/html5/thumbnails/1.jpg)
The Periodic TablePeriodic Properties
![Page 2: Periodic Properties. Atomic Size Atomic size: the radius of an atom (distance from nucleus to electron cloud) is considered. Measured in angstroms (A)](https://reader035.vdocuments.site/reader035/viewer/2022071807/56649e705503460f94b6d72d/html5/thumbnails/2.jpg)
Atomic SizeAtomic size: the radius of an atom (distance
from nucleus to electron cloud) is considered. Measured in angstroms (A) : 1 cm = 1x108 A
•Periodic Trend: Atomic size within a group increases and decreases as atomic number increases. Atomic size increases
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Ionic SizeSome elements tend to gain or lose electrons
to form ions.Metals lose electrons and form positive ions
called cations.Nonmetals gain electrons and form negative
ions called anions.
Fe2+
Iron has a 2+ charge because it lost 2 electons.
![Page 4: Periodic Properties. Atomic Size Atomic size: the radius of an atom (distance from nucleus to electron cloud) is considered. Measured in angstroms (A)](https://reader035.vdocuments.site/reader035/viewer/2022071807/56649e705503460f94b6d72d/html5/thumbnails/4.jpg)
Ionic SizePeriodic Trend:
Cations are smaller than original atom. Losing electrons means the nucleus has a greater attraction for electrons remaining.
Anions are bigger than original atom. Gaining electrons means the nucleus has less attraction for a greater number of electrons.
![Page 5: Periodic Properties. Atomic Size Atomic size: the radius of an atom (distance from nucleus to electron cloud) is considered. Measured in angstroms (A)](https://reader035.vdocuments.site/reader035/viewer/2022071807/56649e705503460f94b6d72d/html5/thumbnails/5.jpg)
Learning CheckFor each of the following sets of atoms and
ions, decide which is the smallest.a. Na, Na+
b. Cl, Cl-
c. Na+, Cl-
d. H+, H, H-
e. Fe2+, Fe3+
f. F-, Ne, Na+
![Page 6: Periodic Properties. Atomic Size Atomic size: the radius of an atom (distance from nucleus to electron cloud) is considered. Measured in angstroms (A)](https://reader035.vdocuments.site/reader035/viewer/2022071807/56649e705503460f94b6d72d/html5/thumbnails/6.jpg)
Learning CheckFor each of the following sets of atoms and
ions, decide which is the smallest.a. Na, Na+
b. Cl, Cl-
c. Na+, Cl-
d. H+, H, H-
e. Fe2+, Fe3+
f. F-, Ne, Na+
![Page 7: Periodic Properties. Atomic Size Atomic size: the radius of an atom (distance from nucleus to electron cloud) is considered. Measured in angstroms (A)](https://reader035.vdocuments.site/reader035/viewer/2022071807/56649e705503460f94b6d72d/html5/thumbnails/7.jpg)
ClassworkTextbook p 255 #1,2
p 257 # 3,4 p 266 # 19
![Page 8: Periodic Properties. Atomic Size Atomic size: the radius of an atom (distance from nucleus to electron cloud) is considered. Measured in angstroms (A)](https://reader035.vdocuments.site/reader035/viewer/2022071807/56649e705503460f94b6d72d/html5/thumbnails/8.jpg)
Ionization energyEnergy required to remove an electron from
an atom.Measured when element is in gaseous state.
First ionization energy: energy required to remove first electron from the highest occupied energy level.
Measured in kJ/molSome elements have second, third…
ionization energy, meaning they can lose more than one electron forming positive ions.
![Page 9: Periodic Properties. Atomic Size Atomic size: the radius of an atom (distance from nucleus to electron cloud) is considered. Measured in angstroms (A)](https://reader035.vdocuments.site/reader035/viewer/2022071807/56649e705503460f94b6d72d/html5/thumbnails/9.jpg)
Trends in ionization energyIonization energy increases
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Trends in ionization energy
Ionization energy increases
Ionization energy increases within a period.As the number of protons increases, the nuclear force increases making harder to remove an electron.
Ionization energy decreases within a group.As the size of the atom increases, nuclear force has a smaller effect on electrons on highest energy level.
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ElectronegativityIs the ability of an element to attract
electrons when the atom is in a compound.Noble gases are omitted because they don’t
form many compounds.Most electronegative element is FluorineLeast electronegative element is cesium
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Trends in electronegativityElectronegativity increases
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