10. Periodic Properties of the Elements

Periodic Trend: Ionization Energy

in terms of ionization energy. The periodic trend is ionization. Energy will increase as we're moving from left to right across a period and upper group. So as we're heading towards the upper right corner of the periodic table, ionization energy goes up here. If we take a look, we can see that the one with lowest ionization energy is Francie um, which makes the most sense because it's on the exact opposite, um, pattern of the periodic trend. And we can see here that the one with the highest is helium. It's to the most top right corner of the periodic table. Now, of course, there's gonna be a little bit of, um, some exceptions to this trend. We'll go into further detail about them. You'll notice here that nitrogen has a lower, higher ionization energy than oxygen. You also notice here that beryllium has, ah higher ionization energy than boron. There are other little subtle exceptions, but these four elements are the most commonly discussed when it comes to exceptions in ionization energy. So just realize that overall, as we head to the top right corner of the periodic table, ionization energy goes up

Periodic Trends: Electronegativity, Ionization Energy, Atomic Radius, and Electron Affinity

Electronegativity and Ionization Energy

Choose the element with the higher first ionization energy 
from each pair. 
d. P or Sn

The Periodic Table EXPLAINED | Chemical Families and Periodic Trends

One way to measure ionization energies is ultraviolet photoelectron
spectroscopy (PES), a technique based on the
photoelectric effect. (Section 6.2) In PES, monochromatic
light is directed onto a sample, causing electrons to
be emitted. The kinetic energy of the emitted electrons is
measured. The difference between the energy of the photons
and the kinetic energy of the electrons corresponds to the
energy needed to remove the electrons (that is, the ionization
energy). Suppose that a PES experiment is performed
in which mercury vapor is irradiated with ultraviolet light
of wavelength 58.4 nm. (d) Using Figure 7.10, determine which of the halogen 
elements has a first ionization energy closest to that 
of mercury.

One way to measure ionization energies is ultraviolet photoelectron
spectroscopy (PES), a technique based on the
photoelectric effect. (Section 6.2) In PES, monochromatic
light is directed onto a sample, causing electrons to
be emitted. The kinetic energy of the emitted electrons is
measured. The difference between the energy of the photons
and the kinetic energy of the electrons corresponds to the
energy needed to remove the electrons (that is, the ionization
energy). Suppose that a PES experiment is performed
in which mercury vapor is irradiated with ultraviolet light
of wavelength 58.4 nm. (c) The kinetic energy of the emitted electrons is measured to be 1.72 * 10-18 J. What is the first ionization energy of Hg, in kJ>mol?

The ionization energy of an atom can be measured by photo-electron spectroscopy, in which light of wavelength l is directed at an atom, causing an electron to be ejected. The kinetic energy of the ejected electron 1EK2 is measured by determining its velocity, v since EK = 1/2 mv2. The Ei is then calculated using the relationship that the energy of the inci-dent light equals the sum of Ei plus EK. 
(a) What is the ionization energy of rubidium atoms in kilo-joules per mole if light with l = 58.4 nm produces elec-trons with a velocity of 2.450 * 106m/s? (The mass of an electron is 9.109 * 10-31 kg.)

Rank the following elements in order of increasing ionization energy:Br, F, Ga, K and Se.

Which of the following has the highest ionization energy?&nbsp;

Trends in the Periodic Table

It is possible to define metallic character as we do in this book
and base it on the reactivity of the element and the ease with
which it loses electrons. Alternatively, one could measure
how well electricity is conducted by each of the elements to
determine how “metallic” the elements are. On the basis of
conductivity, there is not much of a trend in the periodic table:
Silver is the most conductive metal, and manganese the
least. Look up the first ionization energies of silver and manganese;
which of these two elements would you call more
metallic based on the way we define it in this book?

Which of the following chemical equations is connected to
the definitions of (a) the first ionization energy of oxygen
(i) O1g2 + e-¡O-1g2 (ii) O1g2¡O+1g2 + e-
(iii) O1g2 + 2 e-¡O2-1g2 (iv) O1g2¡O2+1g2 + 2 e-
(v) O+1g2¡O2+1g2 + e-

Choose the element with the higher first ionization energy 
from each pair. 
a. Br or Bi

The first ionization energy of the oxygen molecule is the energy
required for the following process:
O21g2¡O2 +1g2 + e-
The energy needed for this process is 1175 kJ>mol, very similar
to the first ionization energy of Xe. Would you expect O2 to react
with F2? If so, suggest a product or products of this reaction.

Consider the electronic structure of the element bismuth.
(d) Would you expect element 115 to have an ionization ene-rgy greater than, equal to, or less than that of bismuth? Explain.

Ionization Energy involves an endothermic process where energy is absorbed when electron is removed.

Arrange these elements in order of increasing first ionization 
energy: Si, F, In, N.

Identify each statement as true or false:
(a) Ionization energies are always endothermic.
(b) Potassium has a larger first ionization energy than lithium.
(c) The second ionization energy of the sodium atom is larger than the second ionization energy of the magnesium atom.
(d) The third ionization energy is three times the first ionization energy of an atom.

Based on their positions in the periodic table, predict which
atom of the following pairs will have the smaller first ionization
energy: (d) Pb, S

Choose the element with the higher first ionization energy 
from each pair. 
c. As or At

Moving towards the top right corner of the Periodic Table causes ionization energy to increase.

Choose the element with the higher first ionization energy 
from each pair. 
b. Na or Rb

Consider this set of ionization energies. 
IE1 = 578 kJ>mol 
IE2 = 1820 kJ>mol 
IE3 = 2750 kJ>mol 
IE4 = 11,600 kJ>mol 
To which third-period element do these ionization values belong?

The Periodic Table: Atomic Radius, Ionization Energy, and Electronegativity

(b) Which element in
the periodic table has the largest ionization energy? Which
has the smallest?

Periodic Trend: Ionization Energy Example 1

When in same period, Group 3A elements have lower IE&nbsp;than Group 2A elements due to s subshell orbitals being more stable when totally filled.

When in same period, Group 6A elements have lower IE than Group 5A elements due to p subshell orbitals being more stable half-filled or totally filled.

 Removal of the second electron from P does not involve a core electron. 

 Removal of the second electron from Si does not involve a core electron. 

 Removal of the second electron from Al does not involve a core electron. 

 Removal of the second electron from Mg does not involve a core electron. 

 Correct, removing the second electron from Na involves breaking into a noble gas core electron configuration. 

 The removal of a core electron requires a very large input of energy. 

Which of the following has the largest second ionization energy?

Choose the element with the higher first ionization energy from each pair. 
a. P or I 
b. Si or Cl 
c. P or Sb 
d. Ga or Ge

Ionization Energy and Atomic Radius

Write equations that show the processes that describe the
first, second, and third ionization energies of a chlorine
atom. Which process would require the least amount of
energy?

Write equations that show the process for (a) the first two
ionization energies of zinc (b) the fourth ionization 
energy of calcium.

Periodic Trends: Electronegativity, Ionization Energy, Atomic Radius - TUTOR HOTLINE

The energy of an electron in a one-electron atom or ion equals (–2.18 x 10–18 J) (Z2/n2). Estimate the ionization energy for the valence electron of the Li atom and compare it to its theoretical value.

Periodic Trends: Ionization Energy

Modern Atomic Theory: Ionization Energy

 Correct, since Si is closer to the lower left-side of the periodic table, it has the lowest ionization energy in this series. 

 In determining the order of this series, the alkaline earth metals will have higher values than the corresponding alkali metals. 

 Ionization energy increases as you move across a period from left to right and decreases down a group of the periodic table. 

 Which of the following lists the atoms in order of increasing ionization energy (smallest to largest)? 

Mercury in the environment can exist in oxidation states 0,
+1, and +2. One major question in environmental chemistry
research is how to best measure the oxidation state of mercury
in natural systems; this is made more complicated by the
fact that mercury can be reduced or oxidized on surfaces differently
than it would be if it were free in solution. XPS, X-ray
photoelectron spectroscopy, is a technique related to PES (see
Exercise 7.111), but instead of using ultraviolet light to eject valence
electrons, X rays are used to eject core electrons. The energies
of the core electrons are different for different oxidation
states of the element. In one set of experiments, researchers
examined mercury contamination of minerals in water. They
measured the XPS signals that corresponded to electrons ejected
from mercury’s 4f orbitals at 105 eV, from an X-ray source
that provided 1253.6 eV of energy 11 ev = 1.602 * 10-19J2.
The oxygen on the mineral surface gave emitted electron energies
at 531 eV, corresponding to the 1s orbital of oxygen.
Overall the researchers concluded that oxidation states were
+2 for Hg and -2 for O. (b) Compare the energies of
the 4f electrons in mercury and the 1s electrons in oxygen
from these data to the first ionization energies of mercury
and oxygen from the data in this chapter.

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1. Intro to General Chemistry

2. Atoms & Elements

3. Chemical Reactions

4. BONUS: Lab Techniques and Procedures

5. BONUS: Mathematical Operations and Functions

6. Chemical Quantities & Aqueous Reactions

7. Gases

8. Thermochemistry

9. Quantum Mechanics

11. Bonding & Molecular Structure

12. Molecular Shapes & Valence Bond Theory

13. Liquids, Solids & Intermolecular Forces

14. Solutions

15. Chemical Kinetics

16. Chemical Equilibrium

17. Acid and Base Equilibrium

18. Aqueous Equilibrium

19. Chemical Thermodynamics

20. Electrochemistry

21. Nuclear Chemistry

22. Organic Chemistry

23. Chemistry of the Nonmetals

24. Transition Metals and Coordination Compounds

[BOOK CHEM] Clutch Version

Periodic Trend: Cumulative

Periodic Trends are patterns present in the periodic table based on an element's size and electron distribution.&nbsp;

Periodic Trend: Ionic Radius

Ionic Radius is the distance between an ion's nucleus and its most outer occupied electron shell.&nbsp;

The Electron Configuration

The electron configuration of an element is the distribution of its electrons within atomic orbitals.&nbsp;

The Electron Configuration: Ions

The Electron Configuration of Ions involves either adding or removing electrons from a given orbital of an element.

Periodic Trend: Successive Ionization Energies

Successive Ionization Energies deals with the removal of multiple electrons from a gaseous atom or ion through multiple steps.

Periodic Trend: Atomic Radius

The atomic radius of an element is the distance from its nucleus to its outer electron shell.

Valence Electrons of Elements

The Valence Electrons represent the outer shell electrons of an element or ion.&nbsp;

Periodic Trend: Effective Nuclear Charge

Effective Nuclear Charge (Zeff) measures the force exerted onto an electron by the nucleus.&nbsp;

Ionization Energy is the energy absorbed&nbsp;in order to remove an electron from a gaseous atom or ion.&nbsp;

Periodic Trend: Metallic Character

Metallic Character&nbsp;deals with how easily an electron can be removed from an element.&nbsp;

Paramagnetism and Diamagnetism

Paramagnetism&nbsp;and&nbsp;Diamagnetism deal with the presence of electrons that are either unpaired or paired in an orbital.

Periodic Trend: Electron Affinity

Electron Affinity is the energy released from the addition of an electron to a gaseous atom or ion.&nbsp;

The Electron Configuration: Quantum Numbers

The Quantum Numbers ultimately can be used to determine the precise location of an electron.&nbsp;

Periodic Trend: Electronegativity

Electronegativity is an element's ability to attract electrons.

The Electron Configurations: Exceptions

Most Electron Configuration Exceptions are the result of elements drive to obtain half filled or totally filled d orbitals.&nbsp;

The Electron Configuration: Condensed

Condensed Electron Configurations are a faster method in determining the configuration of elements and ions.&nbsp;