Problem: How many electrons in an atom can have the designation 1p, 6dx2 - y2, 4f, 7py, 2s, n = 3?

FREE Expert Solution

1p

• when n = 1

• l = 0 only → s orbital

• 1p does not exist 

no electrons


6dx- y2

• l = 2 only → d orbital

• ml = -2, -1 , 0, 1, 2

d orbitals = dz2, dxy, dyz, and dx2-y2

1 orbital = max. of 2 electrons

• 6dx- y2 → 2 electrons


4f

• l = 3 → f orbital

• ml = -3, -2, -1 , 0, 1, 2, 3

f orbitals = 7 orbtials

1 orbital = max. of 2 electrons

• 4f → 14 electrons


7py

• l = 1 → p orbital

• ml =  -1 , 0, 1

p orbitals = px, py, pz

1 orbital = max. of 2 electrons

• 7py → 2 electrons

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Problem Details

How many electrons in an atom can have the designation 1p, 6dx- y2, 4f, 7py, 2s, n = 3?

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What scientific concept do you need to know in order to solve this problem?

Our tutors have indicated that to solve this problem you will need to apply the Quantum Numbers: Number of Electrons concept. You can view video lessons to learn Quantum Numbers: Number of Electrons. Or if you need more Quantum Numbers: Number of Electrons practice, you can also practice Quantum Numbers: Number of Electrons practice problems.

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Based on our data, we think this problem is relevant for Professor Hummel's class at UIUC.

What textbook is this problem found in?

Our data indicates that this problem or a close variation was asked in Chemistry: An Atoms First Approach - Zumdahl Atoms 1st 2nd Edition. You can also practice Chemistry: An Atoms First Approach - Zumdahl Atoms 1st 2nd Edition practice problems.