Question 1

Which of the following statements best explains why potassium ions (K$$^+) $$and sodium ions (Na$$^+) $$can be selectively transported across cell membranes, even though both are 1+ cations?

Accepted Answer

Cell membranes are sensitive to the difference in ionic size between K$$^+$$ and Na$$^+$$, allowing selective transport.

Question 2

According to the Pauli Exclusion Principle, what is the maximum number of electrons that can occupy a single orbital?

Accepted Answer

$$2$$

Question 3

Which quantum number is responsible for distinguishing the two electrons in the same orbital?

Accepted Answer

Spin quantum number $$m_s$$

Question 4

What is the electron configuration for nitrogen (N), which has 7 electrons?

Accepted Answer

$$1s^2$$ $$2s^2$$ $$2p^3$$

Question 5

Which of the following best describes a periodic property?

Accepted Answer

A property that is predictable based on an element's position in the periodic table.

Question 6

How many valence electrons does a fluorine atom have?

Accepted Answer

$$7$$

Question 7

Which principle states that orbitals of identical energy are each occupied singly before any orbital is doubly occupied?

Accepted Answer

Hund's Rule

Question 8

What is the electron configuration for lithium (Li)?

Accepted Answer

$$1s^2$$ $$2s^1$$

Question 9

Which of the following sublevels can hold a maximum of 10 electrons?

Accepted Answer

d sublevel

Question 10

If an atom has the electron configuration $$[Ne]3s^2$ 3p^5$, how many valence electrons does it have?

Accepted Answer

$$7$$

Question 11

Which of the following best describes the order in which orbitals are filled in multielectron atoms?

Accepted Answer

Orbitals fill in order of increasing energy, starting with the lowest energy orbital.

Question 12

Which quantum numbers are needed to uniquely identify an electron in an atom?

Accepted Answer

$$n$$, $$l$$, $$m_l$$, and $$m_s$$

Question 13

Which of the following is true about the energy ordering of orbitals in multielectron atoms?

Accepted Answer

The $$4s$$ orbital lies lower in energy than the $$3d$$ orbitals.

Question 14

Which equation describes the potential energy between two charged particles according to Coulomb's Law?

Accepted Answer

$$E = \frac{q_1$ q_2$}{4 \pi \$$epsilon_0$$ r}$$

Question 15

What is the electron configuration for sulfur (S), which has 16 electrons?

Accepted Answer

$$1s^2$$ $$2s^2$$ $$2p^6$$ $$3s^2$$ $$3p^4$$

Question 16

Which of the following statements about electron penetration and shielding is correct?

Accepted Answer

Electrons that penetrate the electron cloud of inner electrons experience greater attraction to the nucleus.

Question 17

How many electrons can occupy the $$f$$ sublevel?

Accepted Answer

$$14$$

Question 18

Which of the following is the correct set of quantum numbers for the two electrons in a $$4s$$ orbital?

Accepted Answer

$$n=4, l=0, m_l=0, m_s=+1/2$$ and $$n=4, l=0, m_l=0, m_s=-1/2$$

Question 19

Which of the following best explains why elements in the same column of the periodic table have similar chemical properties?

Accepted Answer

They have the same number of valence electrons.

Periodic Properties of the Elements

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