Ionization energy
Moderators: Chem_Mod, Chem_Admin
-
- Posts: 97
- Joined: Sat Jul 20, 2019 12:15 am
Ionization energy
Are we expected to know a specific formula for ionization energy or only the general trends of ionization energy?
-
- Posts: 46
- Joined: Sat Sep 07, 2019 12:16 am
Re: Ionization energy
I think we should know the general trends for ionization energy, not only because he went over it in class but because it's useful for drawing Lewis structures and understanding other topics.
Ionization energy increases as you move across a period and decreases as you move down groups.
Ionization energy increases as you move across a period and decreases as you move down groups.
-
- Posts: 52
- Joined: Wed Sep 18, 2019 12:18 am
Re: Ionization energy
Ionization energy is defined as the minimum amount of energy required to remove the most loosely bound electron from an atom or molecule in gas state. The tighter a molecules radius, the harder to remove an electron from it. Thats how I like to think of it. So as atomic radius increases, ionization energy decreases.
-
- Posts: 58
- Joined: Sat Aug 17, 2019 12:15 am
Re: Ionization energy
The atomic radius generally increases from right to left across a group. It also normally increases top to bottom within a group. I use the periodic table and the inverse relationship between atomic radius and ionization energy to help with ionization energy problems.
-
- Posts: 45
- Joined: Sat Aug 17, 2019 12:16 am
Re: Ionization energy
I think you should know that on the periodic table, ionization energy increases going left to right across a period because atomic radius decreases, so electrons are more closely attracted to the nucleus. Going down a group, ionization energy decreases because valence electrons are shielded further away from the nucleus.
-
- Posts: 101
- Joined: Fri Aug 09, 2019 12:17 am
Re: Ionization energy
It's pretty important to understand the ionization energy trends when looking at a periodic table - ionization energy increases from left to right across a period and decreases move down groups. It is measured in joules (J) or electron volts (eV), and is calculated by subtracting 1 from the atomic number, squaring that value, and multiplying the result by 13.6 (you get the answer in eV).
Ionization energy (of an atom, in eV) = (atomic # - 1)2 x 13.6
Ex: Ionization energy of He = (2-1)2 x 13.6 = 13.6 eV
Ionization energy (of an atom, in eV) = (atomic # - 1)2 x 13.6
Ex: Ionization energy of He = (2-1)2 x 13.6 = 13.6 eV
-
- Posts: 104
- Joined: Thu Jul 25, 2019 12:18 am
Re: Ionization energy
You should understand the trends of ionization energy. It increases going across a period and up a group.
-
- Posts: 112
- Joined: Fri Aug 09, 2019 12:17 am
- Been upvoted: 1 time
Re: Ionization energy
I'm not sure if we'll get into it during this course, but there are some exceptions to the general trend. For example, the elements in group 16 tend to have lower 1st ionization energies than the elements in group 15 due to the fact that group 16 elements have a filled orbital which leads to greater interelectronic repulsions between the two electrons in it.
Re: Ionization energy
Ionization energy is also important when drawing lewis structures as the atom with the lowest ionization energy is typically drawn as the central atom.
-
- Posts: 100
- Joined: Sat Aug 17, 2019 12:18 am
Re: Ionization energy
I believe that it is most important to understand the general trends associated with ionization energy. Ionization energy is said to be the energy needed to remove an electron from an atom in the gas phase. Thus, ionization energy decreases down a group and increases across a period.
-
- Posts: 107
- Joined: Fri Aug 09, 2019 12:17 am
Re: Ionization energy
All you're really supposed to know for Ionization Energies is the trends for lewis structures later.
-
- Posts: 96
- Joined: Wed Nov 21, 2018 12:19 am
Re: Ionization energy
I don't think we have to know the actual equation but rather just the general trend of Ionization Energy in the periodic table.
Return to “Trends in The Periodic Table”
Who is online
Users browsing this forum: No registered users and 5 guests