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

Name: Problem 40, Chapter 7: Chemistry The Central Science
Uploaded: 2019-05-04T14:47:11-08:00
Duration: 4 min 16 s
Channel: James Irizarry
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.

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Key Concepts

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.

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.

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.

Transcript

00:01 All right, guys.

00:01 Return problem number forty in chapter seven of commissioners central science.

00:07 So they want to identify each state mass.

00:08 Truer pulse.

00:09 And we have four four statements here.

00:11 First time in a ionization energies are always negative quantities.

00:15 Well, no, because when it comes to ionization energy, you have to input energy in your system system because the electrons, like teo, be bound, bound in their in their electron cloud because because they're closer to the nucleus and says nucleus possibly charged, you have to as you have to us, you have to input energy to remove those electrons.

00:43 So this is false else.

00:48 You're the ionization, and she's going to be positive.

00:51 Now.

00:52 Be oxygen.

00:53 It has a larger first ionization energy than flooring.

00:58 Well, let's think about this.

00:59 Remember minutes, so oxygen.

01:04 Oh, as so you can tell which one has a first ionization energy by periodic trends.

01:17 So so let's mess.

01:20 So here's our periodic table.

01:24 So so when you go this way, ionization energy increases...