Identify each statement as true or false: (a) Ionization...

Name: Problem 40, Chapter 7: Chemistry The Central Science
Uploaded: 2021-08-26T01:06:14-08:00
Duration: 3 min 54 s
Channel: Tracy Tourville
Description: Identify each statement as true or false: (a) Ionization energies are always negative quantities. (b) Oxygen has a larger first ionization energy than fluorine. (c) The second ionization energy of an atom is always greater than its first ionization energy. (d) The third ionization energy is the energy needed to ionize three electrons from a neutral atom.

Identify each statement as true or false: (a) Ionization energies are always negative quantities. (b) Oxygen has a larger first ionization energy than fluorine. (c) The second ionization energy of an atom is always greater than its first ionization energy. (d) The third ionization energy is the energy needed to ionize three electrons from a neutral atom.

Key Concepts

Successive Ionization Energies

Successive ionization energies are the energies required to remove electrons sequentially from an atom. The second ionization energy is for removing an electron from an atom that has already lost one electron, and it is typically higher than the first ionization energy due to the increased effective nuclear charge on the remaining electrons. Similarly, each subsequent ionization energy further increases and refers to the energy required to remove one electron at a time from the increasingly positive ion.

Periodic Trends in Ionization Energy

Periodic trends in ionization energy refer to the systematic changes observed in the energy required to remove an electron as one moves across periods and down groups in the periodic table. Generally, ionization energy increases across a period due to increasing nuclear charge and decreases down a group due to additional electron shells that increase the distance between the nucleus and the valence electrons.

Ionization Energy

Ionization energy is the amount of energy required to remove an electron from an isolated gaseous atom or ion. This is an endothermic process and is defined as a positive value since energy must be supplied to overcome the electrostatic attraction between the negatively charged electron and the positively charged nucleus.

Transcript

00:01 This question deals with periodic table and some of the periodic properties.

00:05 It especially talks about ionization energy.

00:08 That's the energy required to strip away an electron.

00:12 And we're asked to determine whether the given statements below that i've kind of summarized here are true or false statements.

00:19 And what did i just say about ionization energy? the energy required to strip away a substance.

00:25 It's an endothermic quantity.

00:27 It requires energy to strip away.

00:30 Electrons.

00:32 So it will always be an endothermic process with a positive amount of energy going into the system to strip away an electron.

00:39 So the first statement here saying that ionization energy is negative or an exothermic process is false.

00:46 It's always an endothermic process, always requires energy to strip away electrons.

00:54 Therefore, there always be a positive sign associated with the endothermic process of ionization energy.

01:02 The second statement, asks if the ionization energy of oxygen on the periodic table is greater than fluorine.

01:09 Well, the general trend that we see for ionization energy on the periodic table is, as we move left to right across any row, the ionization energy or energy required to strip away electrons increases.

01:22 We'll check it out here.

01:23 Floring and oxygen are in the same row of the periodic table, but fluorine is to the right of oxygen.

01:29 That means fluorine should have a higher ionization energy than oxygen...

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