QuestionPlace the following in order of increasing .
N
F
As
A)
B)
C)
D)
E) As
Studdy Solution
STEP 1
What is this asking?
Which element, Nitrogen (N), Fluorine (F), or Arsenic (As), is easiest to remove an electron from, and which is hardest?
Watch out!
Don't confuse *ionization energy* with *electron affinity*.
Ionization energy is about *removing* an electron, not *adding* one!
STEP 2
1. Periodic Trends
2. Element Comparison
STEP 3
Ionization energy is the energy needed to remove an electron from an atom.
Think of it like this: how much energy does it take to steal that electron?
A *higher* ionization energy means it's *harder* to remove the electron.
STEP 4
As we move *left to right* across a period (row) in the periodic table, ionization energy generally *increases*.
This is because the number of protons increases, pulling the electrons in tighter.
It's like adding more magnets to hold onto those electrons!
STEP 5
As we move *down* a group (column), ionization energy generally *decreases*.
This is because electrons are further away from the nucleus in larger atoms, and those outer electrons are shielded from the positive charge by the inner electrons.
It's like trying to grab something from the outer layer of a giant onion – easier than grabbing from the core!
STEP 6
Let's find our elements on the periodic table!
Nitrogen () is in period 2, group 15.
Fluorine () is in period 2, group 17.
Arsenic () is in period 4, group 15.
STEP 7
Both and are in the same period (row).
Since is to the *right* of , has a *higher* ionization energy.
It's harder to steal an electron from than from .
So, .
STEP 8
Nitrogen () and Arsenic () are in the same group (column).
Since is *below* , has a *lower* ionization energy.
It's easier to steal an electron from than from .
So, .
STEP 9
We know and .
Combining these, we get .
STEP 10
The correct order of increasing first ionization energy is , which corresponds to answer choice **B**.
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