4.4 - 5.10

List the following elements in order of decreasing atomic radius (largest at the top to smallest at the bottom). Li, N, He, B

1. Li 2. B 3. N 4. He

Arrange the following elements in order of increasing ionization energies (lowest at the top, highest at the bottom) based on periodic trends. Ca, K, Br, Rb

1. Rb 2. K 3. Ca 4. Br

Arrange the following elements in order of increasing atomic size, starting with the smallest atom at the top of the list. Se, Br, S, I

1. S 2. Br 3. Se 4. I

Which of the following options correctly describe metallic character? Select all that apply.

A tendency to lose electrons and form cations High electrical and thermal conductivity

Which of the following statements correctly describe atomic radii? Select all that apply.

Atomic radii of main group elements decrease from Group 1A to Group 8A. Atomic radii generally increase as n increases.

The energy required for the complete removal of 1 mol of electrons from 1 mol of gaseous atoms or ions is called ___ energy. For a neutral element this energy is a measure of how easily the element forms a(n) ___ , which is an ion with a net ___ charge.

Blank 1: ionization, first ionization, or ionisation Blank 2: cation Blank 3: +, positive, plus, +1, or 1+

The ___ radius is defined as half the separation between two adjacent, identical metal atoms. The ___ radius is defined as half the separation between two bonded identical nonmetal atoms.

Blank 1: metallic Blank 2: covalent or bonding

Why does ionization energy generally increase from left to right across a period?

Effective nuclear charge increases and the outermost electron becomes harder to remove.

Which of the following statements correctly describe electron affinity? Select all that apply.

Electron affinity is the energy released during the addition of 1 mol of electrons to 1 mol of gaseous atoms or ions. Electron affinity measures the tendency of an element to form an anion. The overall trend in electron affinities is to increase from left to right across a period.

In each of the following pairs of elements, select the element that will have the greater value for electron affinity.(i) Li vs. F(ii) P vs. S

F; S

Match the trends in ionization energies correctly.

IE decreases --> down a group IE increases --> from left to right across a period

Which of the following statements describe/define ionization energy correctly? Select all that apply.

Ionization energy is the energy (kJ) required for the complete removal of 1 mol of valence electrons from 1 mol of gaseous atoms or ions. The ionization energy of an element is a measure of how easily it forms a cation.

Match each of the following elements with the correct number of electrons lost or gained to form its most common ion.

K - loses one electron Cl - gains 1 electron Mg - loses 2 electrons S - gains 2 electrons

Match each type of element with the typical trend it follows when forming an ion. Instructions

Main group s-block metals -- lose all electrons from ns sublevel Main group p-block metals -- lose first the np electrons, then the ns electrons main group nonmetals -- gain electrons to fill the np sublevel transition metals -- lose ns electrons before losing (n-1)d electrons

Which of the following statements correctly describe metallic character and its general trends? Select all that apply.

Metallic character increases down a group. Metallic character decreases from left to right in a period.

Which of the following options correctly describe the general trends followed by elements when they form ions? Select all that apply.

Metals generally form cations. The charge of a main group cation is equal to its group number. Noble gases do not usually form ions.

Which element has the lowest second ionization energy?

Mg

Why does atomic radius generally increase down a group on the periodic table?

Moving down a group, the outer electrons are at increasingly higher energy levels, causing them to be farther from the nucleus.

Which of the following elements is expected to have the highest first ionization energy, based on periodic trends?

Ne Reason: Ionization energy is closely related to effective nuclear charge. Ne is in Period 2 and its outermost electrons are therefore in the second principal energy level or shell. It is harder to remove one of these electrons than to remove an electron from the third principal energy level.

Which of the following statements correctly describe the trends in ionization energy (IE)? Select all that apply.

Noble gases have high ionization energies. Atoms with low ionization energies tend to form cations.

Which of the following monatomic ions have the electron configuration 1s22s22p6? Select all that apply.

O2- Na+ F-

Which element, S or P, will have the higher first ionization energy, and why? Select the statement that best describes the reason for your choice. (Hint: in order to answer this question, first write out the electron configurations for both elements.)

P will have a higher first ionization energy.` Removing an electron from P is more difficult because all outermost electrons are unpaired, whereas there are two paired outermost electrons in S.

Which element, Si or P, will have a higher electron affinity, and why? Select both the element and the reason for its behavior.(Hint: write out the electron configuration for each element before answering the question, and pay particular attention to the number of unpaired electrons present.)

P will have a lower value for electron affinity because the electron gained would be placed in an orbital that already contains an electron. Si will have a greater value for EA.

Which element, Mg or Al, will have the higher first ionization energy, and why? Select the statement that best describes the reason for your choice. (Hint: in order to answer this question, first write out the electron configurations for both elements.)

Removing an electron from Mg is more difficult because the outermost electron is in a lower-energy ns orbital. Mg will have a higher first ionization energy.

Na has a higher electron affinity than Mg, which is contrary to the usual trend. Which of the following statements correctly explain this anomaly? Select all that apply.

The extra electron added to Na will fill its s subshell, which is favorable. The extra electron added to Na will be placed in a lower energy orbital than the extra electron added to Mg.

Select the correct electron configuration for Sn4+.

[Kr]4d^10

The atomic radius of an element may differ depending on how it is measured. Match each type of radius in the illustration with the correct description.

a --> metallic radius (grey grid) b --> covalent radius (red cheeks)

In general for main group elements atomic radii _____ from left to right across a period and _____ down a group of the periodic table.

decrease, increase

Ionization energy generally decreases down a group because as one moves down a group, the outermost electron moves _____ the nucleus and it takes _____ energy to remove it.

farther away from; less

Second ionization energies are always _____ than first ionization energies because the remaining electrons are attracted _____ strongly as the positive charge on the ion increases. A large jump in ionization energies is always observed after the _____ electrons have been removed.

higher; more; valence

Atomic radius generally decreases from left to right across a period because the effective nuclear charge ______ while electrons are being added to the same outer shell. These additional electrons are not shielded as well by inner electrons and are therefore attracted ______ strongly by the nucleus.

increases, more

Match each type of element correctly to its characteristic properties

metals - low ionization energies nonmetals - high electron affinities metalloids - intermediate values for electron affinities and ionization energies