GRADE 9 QUIZ

WHICH OF THE FOLLOWING REFERS TO THE DISTANCE OF AN ELECTRON FROM THE NUCLEUS? It is also known as the principal quantum number.

• A. SHELL

• B. SUBSHELL

• C. SPIN

• D. ELECTRON VALENCE

WHICH OF THE FOLLOWING STATEMENTS IS TRUE ABOUT ORBITALS?

• A. EACH ORBITAL CAN HOLD A MAXIMUM OF TWO ELECTRONS.

• B. THE TOTAL NUMBER OF ORBITALS IS A SHELL IS DEPENDENT ON THE DIRECTION OF THE ELECTRONS.

• C. EACH ORBITAL CAN HOLD A MAXIMUM OF 2n2 ELECTRONS

• D. NONE OF THESE

How do you know an element’s principal quantum number easily?

• A. atomic number of the element

• B. period number of the element

• C. mass number of the element

• D. group number of the element

What is the location of an electron with the following set of quantum numbers?

{n=5,ℓ=3,mℓ=−3,ms=+12}

• A. 5f orbital with a positive spin

• B. 5p orbital with a positive spin

• C. 5d orbital with a positive spin

• D. 5s orbital with a positive spin

The lone valence electron of sodium (n=3) will have which set of quantum numbers?

• A. {n=3,ℓ=0,mℓ=0,ms=+12}

• B. {n=3,ℓ=1,mℓ=0,ms=+12}

• C. {n=3,ℓ=2,mℓ=0,ms=+12}

• D. {n=3,ℓ=3,mℓ=0,ms=+12}

What is the location of an electron with the following set of quantum numbers?

{n=5,ℓ=3,mℓ=−3,ms=+12}

• A. 5f orbital with a positive spin

• B. 5p orbital with a positive spin

• C. 5d orbital with a positive spin

• D. 5s orbital with a positive spin

How many electrons in its valence shell can an element hold if it theoretically belongs to period 7?

• A. 98 electrons

• B. 196 electrons

• C. 49 electrons

• D.

  10 electrons

Each subshell has a specific number of atomic orbitals. If an h subshell were to be discovered following the f and g subshells, how many orbitals will it have?

11 orbitals

10 orbitals

15 orbitals

20 orbitals

• A. 11 orbitals

• B. 10 orbitals

• C. 15 orbitals

• D. 20 orbitals

An electron in its ground state has the following set of quantum numbers: {n=1,ℓ=0,mℓ=0,ms=+12}. Upon excitation by light, which state would it transition to? Choose the correct answer.

• a. {n=2,ℓ=0,mℓ=0,ms=+12}

• b.

  {n=1,ℓ=0,mℓ=0,ms=+12}

• c.

  {n=2,ℓ=0,mℓ=0,ms=−12}

• d.

  {n=1,ℓ=0,mℓ=0,ms=−12}