GenChem 1 Flashcards
Which quantum number tells us the shape or the region an electron occupies?
A. Angular Momentum Quantum Number
B. Principal Quantum Number
C. Magnetic Quantum Number
A. Angular Momentum Quantum Number
Which quantum number relates to the average distance of the electron from the nucleus in a particular orbital?
A. Angular Momentum Quantum Number
B. Principal Quantum Number
C. Magnetic Quantum Number
B. Principal Quantum Number
How many possible values of ml are there if l=1?
3
How many possible values of ml are there if l=2?
5
Which of the following is NOT a valid set of quantum numbers?
A. 2,1,0,-1/2
B. 3,3,-2,-1/2
C. 2,1,-1,1/2
D. 4,3,2,1/2
B. 3,3,-2,-1/2
5,5,5,1/2 is not a valid set of quantum numbers. Which of the following is not correct?
A. It is not valid because there is no equivalent orbital for l=5. The equivalent values of l for each orbital are 0=s, 1=p, 2=d, and 3=f.
B. It is not valid because there are three quantum numbers with the value of 5. It can only have two equal values of quantum numbers and that should only be in l and ml.
C. It is not valid because the value of principal quantum number (n) should not be equal to the value of the angular momentum quantum number (l). If l=4, then n should be greater than 4.
D. It is not valid because the value of angular momentum quantum number (l) should not be equal to the value of the principal quantum number (n). The value of the angular momentum quantum number (l) should be less than the value of principal quantum number.
A. It is not valid because there is no equivalent orbital for l=5. The equivalent values of l for each orbital are 0=s, 1=p, 2=d, and 3=f.
There is an equivalent orbital for l=5.
0=s
1=p
2=d
3=f
4=g
5=h
Why are quantum numbers important?
Quantum numbers describe the atomic orbitals and the distribution of electrons in an atom.
What is a paramagnetic substance?
A material that contain net unpaired spins and are attracted by a magnet.
What is a diamagnetic substance?
A material that do not contain net unpaired spins and are slightly repelled by a magnet.
What is the magnetic property of an atom with an electron configuration of 1s2 2s2 2p1?
A. Paramagnetic, because there are no unpaired electrons in its orbital diagram.
B. Diamagnetic, because there are no unpaired electrons in its orbital diagram.
C. Paramagnetic, because there are unpaired electrons in its orbital diagram.
D. Diamagnetic, because there are unpaired electrons in its orbital diagram.
C. Paramagnetic, because there are unpaired electrons in its orbital diagram.
Which among the electron configurations follow the Aufbau principle?
A. 1s2 2s1 2p1
B. 1s2 2s2 2p1
C. 1s2 2s2 2p3 3s1
D. 1s2 2s2 2p3 3s2
B. 1s2 2s2 2p1
According to Aufbau principle, electrons are added in the atomic orbitals from lowest energy to highest energy.
What rule states that no two electrons in an atom can have the same four quantum numbers?
Pauli Exclusion Principle
A cation is formed when an atom loses electron. Which of the following is NOT CORRECT?
A. sodium loses one electron forming a 1+ charge.
B. fluorine gains one electron forming 1- charge.
C. soidum is in group 1 that is why it has 1 valence electrons.
D. fluorine is in period 2 so it can occupy more than 8 electrons
D. fluorine is in period 2 so it can occupy more than 8 electrons
Period 2 elements cannot have an expanded octet.
An anion is formed when an atom gains electron. Which of the following is CORRECT?
A. oxygen forms a cation with a 2- charge.
B. oxygen is found in group 7 in the periodic table.
C. The noble gas configuration of oxygen is equal to the electron configuration of helium.
D. The noble gas configuration of oxide ion (O2-) is equal to the electronic configuration of neon.
D. The noble gas configuration of oxide ion (O2-) is equal to the electronic configuration of neon.
The noble gas configuration of oxide ion is [He] 2p6 which is equivalent to the electronic configuration of neon 1s2 2s2 2p6.
What does the octet rule state in the context of molecular covalent compounds?
Elements tend to form compounds with eight valence electrons.