Using Heisenberg’s uncertainty principle, calculate the uncertainty in the position of b. a proton moving at a speed of (5.00±0.01) × 104 m/s. The mass of a proton is 1.673×10−27 kg.

Calculate the uncertainty in the position of (a) an electron moving at a speed of 13.00 ± 0.012 × 10⁵ m/s (b) a neutron moving at this same speed. (The masses of an electron and a neutron are given in the table of fundamental constants in the inside cover of the text.)

(a) For n = 4, what are the possible values of l?

How many unique combinations of the quantum numbers l and 𝑚𝑙 are there when b. n = 4?

Give the numerical values of n and l corresponding to each of the following orbital designations: (a) 3p (b) 2s (c) 4f

Give the numerical values of n and l corresponding to each of the following orbital designations: (d) 5d.

Give the values for n, l, and 𝑚𝑙 for a. each orbital in the 2p subshell

A certain orbital of the hydrogen atom has n = 4 and l = 2. a. What are the possible values of ml for this orbital?

A certain orbital of the hydrogen atom has n = 4 and l = 2. b. What are the possible values of ms for the orbital?

Which of the following represent impossible combinations of n and l? (a) 1p (b) 4s (c) 5f (d) 2d

For the table that follows, write which orbital goes with the quantum numbers. Don't worry about x, y, z subscripts. If the quantum numbers are not allowed, write 'not allowed.' n l ml Orbital 2 1 -1 2p (example) 1 0 0 3 -3 2 3 2 -2 2 0 -1 0 0 0 4 2 1 5 3 0

Sketch the shape and orientation of the following types of orbitals: (a) s, (b) p_z, (c) d_xy.

Sketch the shape and orientation of the following types of orbitals: (a) p_x, (b) d_z2, (c) d_{x2 - y2}.

(a) With reference to Figure 6.19, what is the relationship between the number of nodes in an s orbital and the value of the principal quantum number?

(a) For an He+ ion, do the 2s and 2p orbitals have the same energy? If not, which orbital has a lower energy?

(b) If we add one electron to form the He atom, would your answer to part (a) change?

(a) The average distance from the nucleus of a 3s electron in a chlorine atom is smaller than that for a 3p electron. In light of this fact, which orbital is higher in energy?

Two possible electron configurations for an Li atom are shown here. (c) In the absence of an external magnetic field, can we say that one electron configuration has a lower energy than the other? If so, which one has the lowest energy?

An experiment called the Stern–Gerlach experiment helped establish the existence of electron spin. In this experiment, a beam of silver atoms is passed through a magnetic field, which deflects half of the silver atoms in one direction and half in the opposite direction. The separation between the two beams increases as the strength of the magnetic field increases. (a) What is the electron configuration for a silver atom?

An experiment called the Stern–Gerlach experiment helped establish the existence of electron spin. In this experiment, a beam of silver atoms is passed through a magnetic field, which deflects half of the silver atoms in one direction and half in the opposite direction. The separation between the two beams increases as the strength of the magnetic field increases. (c) Would this experiment work for a beam of fluorine (F) atoms?

What is the maximum number of electrons that can occupy each of the following subshells? a. 3p, b. 5d, c. 2s, d. 4f.

What is the maximum number of electrons in an atom that can have the following quantum numbers? a. n = 3, ml = -2; b. n = 4, l = 3; c. n = 5, l = 3, ml = 2; d. n = 4, l = 1, ml = 0.

(a) What are 'valence electrons'?

(b) What are 'core electrons'?

(c) What does each box in an orbital diagram represent?

For each element, indicate the number of valence electrons, core electrons, and unpaired electrons in the ground state: a. nitrogen

For each element, indicate the number of valence electrons, core electrons, and unpaired electrons in the ground state: c. chlorine

Write the condensed electron configurations for the following atoms and indicate how many unpaired electrons each has: (a) Mg (b) Ge (c) Br (d) V (e) Y.

Write the condensed electron configurations for the following atoms and indicate how many unpaired electrons each has: (f) Lu.