ORG CHEM QUIZ #1 BSC-E

Which of the following statements is CORRECT about the mass number?

• It is equal to the number of electrons.

• It is the total number of protons and neutrons.

• It is equal to the number of protons.

• It the total number of protons and electrons.

What do you call the atoms with the same atomic number but with different mass numbers?

• Valence electrons

• Cations

• Anions

• Isotopes

What is the probable region of space around the nucleus that an electron is most likely to occupy?

• Orbital

• Valence electron

• Electron shell

• Isotope

What is the maximum number of electrons that can occupy a p orbital?

• 10

• 6

• 2

• 14

What is the representation of the arrangement or distribution of electrons in orbitals around the nucleus?

• Orbital

• Electron configuration

• Lewis eletron-dot structure

• Line-bond structure

Which of the following is TRUE regarding bond formation?

• Making bonds always absorbs energy.

• Breaking bonds always releases energy.

• Atoms prefer to have six electrons in the outer shell to become more stable.

• A stable hydrogen molecule results whenever a noble-gas configuration of two dots is achieved.

Which of the following is TRUE about covalent bonding?

• It involves the transfer of electrons.

• It involves the sharing of electrons.

• Losing an electron will form cations.

• Anions are formed when electrons are accepted.

Which of the following is FALSE about ionic bonding?

• Ionic bonds are formed between metal and non-metals.

• Ionic bonds are formed when there is a big difference in the electronegativity of atoms.

• Ionic bonds are formed when the electronegativity of atoms is similar.

• The type of bond between sodium and chlorine is an ionic bond.

Which of the following is NOT a name of an orbital?

• fundamental

• diffuse

• sharp

• spherical

What does Hund's rule state in the principles of writing the electron configuration?

• The lowest-energy orbitals fill up first.

• Only two electrons can occupy an orbital.

• Electrons must have opposite spins.

• If two or more empty orbitals of equal energy are available, one electron occupies each with spins parallel until all orbitals are half-full.