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MCAT Milesdown Quiz

Quiz generated from MCAT Milesdown

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Question 1

Which atomic model describes the atom as mostly empty space with electrons orbiting a fixed, positively charged nucleus?

Bohr model
Rutherford model
Heisenberg uncertainty principle
Pauli exclusion principle

Question 2

What principle states that it is impossible to know both the momentum and position of an electron simultaneously?

Pauli exclusion principle
Aufbau principle
Heisenberg uncertainty principle
Hund's rule

Question 3

Which rule requires that every orbital in a subshell be singly occupied before any orbital receives a second electron?

Pauli exclusion principle
Hund's rule
Aufbau principle
Heisenberg uncertainty principle

Question 4

What is the maximum number of electrons that can occupy a subshell with azimuthal quantum number l?

2n^2
4l + 2
2l + 1
2l

Question 5

Diamagnetic materials are pulled into an external magnetic field.

True
False

Question 6

Which quantum number describes the three-dimensional shape of an orbital?

Principal quantum number (n)
Azimuthal quantum number (l)
Magnetic quantum number (m_l)
Spin quantum number (m_s)

Question 7

Avogadro's number is equal to ___ particles per mole.

Fill in the blank

Question 8

Which type of bond is formed by the complete transfer of valence electrons between atoms?

Covalent bond
Coordinate covalent bond
Ionic bond
Metallic bond

Question 9

In the Bohr model, electrons orbit the nucleus in orbits that have a fixed size and energy.

True
False

Question 10

What is ionization energy?

Energy released when an electron is added to an atom
Energy required to remove an electron from an atom
Energy required to excite an electron to a higher shell
Energy released when an atom gains a proton

Question 11

Which principle states that no two electrons can have the same four quantum numbers?

Aufbau principle
Pauli exclusion principle
Hund's rule
Heisenberg uncertainty principle

Question 12

What does the principal quantum number n describe?

The 3D shape of the orbital
The electron's energy level or shell
The electron's spin
The orbital's orientation

Question 13

Nonpolar covalent bonds have an electronegativity difference that is:

Less than 0.5
Between 0.5 and 1.7
Greater than 1.7
Equal to 2.0

Question 14

Polar covalent bonds have an electronegativity difference between:

0 and 0.5
0.5 and 1.7
1.7 and 3.3
2.0 and 4.0

Question 15

Which elements most often form hydrogen bonds with hydrogen?

Oxygen, nitrogen, and fluorine
Carbon, hydrogen, and oxygen
Sulfur, phosphorus, and chlorine
Sodium, potassium, and calcium

Question 16

An ion with a positive charge is called a(n):

Cation
Anion
Isotope
Molecule

Question 17

Large, organized arrays of ions are called:

Crystalline lattices
Molecular orbitals
Ionic solutions
Polar molecules

Question 18

Van der Waals forces is a general term that includes:

Dipole-dipole and London dispersion forces
Ionic and covalent bonds
Hydrogen bonds and sigma bonds
Metallic and network forces

Question 19

Dipole-dipole forces occur between:

The positive end of one polar molecule and the negative end of another polar molecule
The positive end of a nonpolar molecule and the negative end of another nonpolar molecule
Ions in a crystalline lattice
Temporary dipoles only

Question 20

London dispersion forces are best described as:

Temporary attractive forces created when a temporary dipole induces a dipole in a neighboring molecule
Permanent attractions between ions
Forces between hydrogen and oxygen, nitrogen, or fluorine
Strong covalent bonds

Question 21

Sigma bonds are formed by:

Head-on overlap between atomic orbitals
Side-to-side overlap between atomic orbitals
Transfer of electrons between atoms
Attraction between ions

Question 22

Polar covalent bonds have an electronegativity difference between 0.5 and 1.7.

True
False

Question 23

Anions carry a positive charge.

True
False

Question 24

Cations are ions with a ___ charge.

Fill in the blank

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