Warm-Up 10/5/2016
Place the following in increasing
atomic size
1. N, Sr, I, Be
2. Li, Hg, Cs, F
3. Fr, Ga, K, Br
Write down the electronic configuration of
the following elements in long hand form
•V
• Zr
•S
• Cr
•I
Ionization Energy
•Ionization Energy is the energy needed to
remove an electron
st
•1 Ionization Energy: energy required to
remove the outermost electron
Ionization Energy
•Ionization Energy depends on:
•a. Distance an electron is from nucleus
•The further the electron is away, the
easier it is to remove
Ionization Energy Continued
Nuclear charge: refers to the attraction
between the nucleus and electrons
•A.K.A the Shielding Effect
•The further away the electrons are, the less
the attraction is between the nucleus and
electrons
•
Trends with
Ionization Energy
•The first Ionization energy
decreases as you move down
a group
•The first Ionization energy
increases as you move across
the periodic table
Ionization Energy Problems
•Arrange the following in terms of increasing
ionization energy:
•A. Li, K, Cs, Na
•B. Ca, Zn, Ge, Br
•C. In, B, Al, Ga
•D. Mg, P, Na, Cl
Practice
•Place the following in increasing Ionization
Energy
•Rb, Mo, Br, Fr
•Cs, O, C, Be, F
•Au, Hf, Ba, Po, At
Electronegativity
•Electronegativity is the tendency of
elements to attract electrons
•Nonmetals attract electrons more than
metals
Electronegativity
•Electronegativity is really the strength of
an element to “steal and keep” electrons
Electronegativity
•Electronegativity is measured on a scale
from 0 to 4
•The most electronegative element is given
a value of 4.0
Electronegativity Continued
•Fluorine is the most electronegative
and given a value of 4.0
•O = 3.5
Cl = 3.0
•S = 2.5
H = 2.1
•Li = 1.0
Na = 0.9
Effects of Electronegativity
•The more electronegative an element is,
the more non-metallic it is
Electronegativity
•The strength of other elements to steal
electrons is compared to the most
electronegative element
Trends in Electronegativity
•Electronegativity increases as you move across
the table
•Electronegativity decreases as you move down
the table
•Electronegativity can be used to predict which
type of bond that atoms will form
Problems
•Arrange the following in terms of
increasing electronegativity:
•a. K, As, Cr, Zn
•b. Sr, Y, Ag, I
•c. F, O, N, Li
•d. Ga, Ca, Fe, K
•e. F, At, Cl, Br
Electron Affinity
• Electron affinity is defined as the neutral atom's
likelihood of gaining an electron.
Electron Affinity of Metals
• Metals have a lower EA than nonmetals
because they give up electrons to have a
stable octet.
Electron Affinity of Nonmetals
•Nonmetals like to gain electrons to
form anions to have a fully stable
octet.
Electron Affinity Trend
•As the you go down the periodic table it
decreases
•As you go across the periodic table it
increases
Review Questions
• Place the following in increasing Electron Affinity
• Na, Rb, Al, P, Cl
• Fr, K, Na, Cs
• K, Mg, Si, S
• Cl, At, I, F
Trends with Ionic Size
•What are Ions?
•Ions form when electrons are gained or
lost
•Metals lose electrons (called Cations) ;
non-metals gain electrons( called
Anions)
Trends with Ionic Size
•The metal ions are
usually smaller than the
metal atoms
•The non-metal ions are
larger than the non-metal
atoms
Ionic Size Trend
•The size of the ions increase
going down the periodic table
•The size of cations decreases as
you move across the table
•The size of anions decreases as
you move across the table
Ionic Size Continued
•Cations are smaller than
their corresponding atoms
+
•Na atom is larger than Na
•Anions are larger than their
corresponding atoms
•F atom is smaller than F
Ionic Size Problems
•State which particle would have
the largest radius in each pair:
•a. Ca, Ca+2
•b. Br, Br
•c. Cl -, Br -,
•d. Na+, K+
Practice
•Place the following in increasing
electronegativity:
•Fr, S, Na, Cl
•Place the following in increasing ionization
energy:
•Cl , As, Ca, Ni
•Place the following in increasing atomic
radius:
•I, Rb, Cs, Ru
For the following pairs of atoms, tell which
one of each pair has the largest ionic radius
a. Al, B
b. S, O
c. Br, Cl
d. Na, Al
e. O, F
For the following pairs of atoms, tell which
one of each pair has the largest ionic radius
a. Al
b. S
c. Br
d. Na
e. O
Indicate which element of the following pairs is
the most electronegative.
a. calcium, gallium
b. lithium, oxygen
c. chlorine, sulfur
d. bromine, arsenic
Indicate which element of the following pairs is
the most electronegative.
a. gallium
b. oxygen
c. chlorine
d. bromine