2-5-2021

Match each of the following elements with the correct number of electrons lost or gained to form its most common ion. K Cl Mg S gains 1 electron

K: loses 1 electron Cl: gains 1 electron Mg: loses 2 electrons S: gains 2 electrons

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

Li B N He

Match each type of element with the typical trend it follows when forming an ion. Main group s-block metals Main group p-block metals Main group nonmetals Transition metals

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.

Rank the following elements in order of increasing metallic character (from least metallic at the top of the list to most metallic at the bottom). Instructions Al P Zn Cs

P Al Zn Cs

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

S Br Se I

True or false: It is possible for a given element to have successive electron affinities. True or False

True

Select the correct electron configuration for Sn4+.

[Kr]4d^10

Which of the following statements correctly describe the trends in ionization energy (IE)? Select all that apply. Multiple select question. a. Atoms with low ionization energies tend to form cations. b. Noble gases have high ionization energies. c. Second ionization energies are always less than first ionization energies. d. Nonmetals tend to have low ionization energies.

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

Which of the following monatomic ions have the electron configuration 1s22s22p6? Select all that apply. a. F^- b. O^ c. S^2- d. Na+ e. Li+

a. F^- b. O^2- d. Na+

Which of the following options correctly describe metallic character? Select all that apply. Multiple select question. a. High electrical and thermal conductivity b. The ability to form either anions or cations easily c. Brittleness in solid phase d. A tendency to lose electrons and form cations

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

Which of the following statements describe/define ionization energy correctly? Select all that apply. Multiple select question. a. 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. b. Ionization energy is the energy required for complete removal of 1 mol of core electrons from 1 mol of gaseous atoms or ions. c. The ionization energy of an element is a measure of how easily it forms an anion. d. The ionization energy of an element is a measure of how easily it forms a cation.

a. 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. d. The ionization energy of an element is a measure of how easily it forms a cation.

Which of the following options correctly describe the general trends followed by elements when they form ions? Select all that apply. a. Noble gases do not usually form ions. b. Metals generally form cations. c. Nonmetals tend to lose electrons. d. The charge of a main group anion is equal to (18 - group number). e. The charge of a main group cation is equal to its group number.

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

Which of the following statements correctly describe electron affinity? Select all that apply. Multiple select question. a. The overall trend in electron affinities is to increase from left to right across a period. b. Electron affinity is the energy released during the addition of 1 mol of electrons to 1 mol of gaseous atoms or ions. c. Most electron affinities are negative. d. Electron affinity measures the tendency of an element to form an anion. e. An element with a high electron affinity will not gain an electron easily.

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

In general for main group elements atomic radii _____ from left to right across a period and _____ down a group of the periodic table. Multiple choice question. a. decrease, increase b. increase, decrease c. increase, increase d. decrease, decrease

a. decrease, increase

A cation is smaller than its parent atom, whereas an anion is larger. Which of the following statements correctly explain this observation? Select all that apply. a. When an anion is formed its radius increases because it gains an electronic energy level. b. A cation is smaller than its parent atom because the attraction of the nucleus for the remaining electrons is greater. c. When an atom gains one or more electrons, its radius increases due to electron-electron repulsions. d. The most common cation formed by a main group element is smaller than its parent atom because it has lost its outer electron shell.

b. A cation is smaller than its parent atom because the attraction of the nucleus for the remaining electrons is greater. c. When an atom gains one or more electrons, its radius increases due to electron-electron repulsions. d. The most common cation formed by a main group element is smaller than its parent atom because it has lost its outer electron shell.

Which of the following statements correctly describe electron affinity? Select all that apply. Multiple select question. a. An element with a high electron affinity will not gain an electron easily. b. Electron affinity is the energy released during the addition of 1 mol of electrons to 1 mol of gaseous atoms or ions. c. Electron affinity measures the tendency of an element to form an anion. d. The overall trend in electron affinities is to increase from left to right across a period. e. Most electron affinities are negative.

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

Which of the following statements correctly describe metallic character and its general trends? Select all that apply. a. The ease with which metals form cations decreases down a group. b. Metallic character increases down a group. c. Metallic character decreases down a group. d. Metallic character decreases from left to right in a period.

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

Which of the following statements describe/define ionization energy correctly? Select all that apply. Multiple select question. a. Ionization energy is the energy required for complete removal of 1 mol of core electrons from 1 mol of gaseous atoms or ions. b. The ionization energy of an element is a measure of how easily it forms a cation. c. The ionization energy of an element is a measure of how easily it forms an anion. d. 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.

b. The ionization energy of an element is a measure of how easily it forms a cation. d. 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.

Metallic character tends to _____ down a group in the periodic table and _____ from left to right across a period. a. decrease, increase b. increase, decrease c. increase, increase d. decrease, decrease

b. increase, decrease

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. a. increases, less b. increases, more c. decreases, more d. decreases, less

b. increases, more

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 a. F; P b. Li; S c. F; S d. Li; P

c. F; S

Why does atomic radius generally increase down a group on the periodic table? a. Electron-electron repulsions become stronger the farther away from the nucleus the electrons are located. b. The charge on the nucleus decreases and the outer electrons are therefore attracted less strongly. c. Moving down a group, the outer electrons are at increasingly higher energy levels, causing them to be farther from the nucleus.

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

Which one of the following statements about successive electron affinities (the stepwise addition of more than one electron to an atom) is correct? a. Successive electron affinities occur with increasing outputs of energy. b. Successive electron affinities do not occur because of the repulsive energy between an incoming electron and an anion. c. Successive electron affinities are possible but require significant energy to occur.

c. Successive electron affinities are possible but require significant energy to occur.

Why does ionization energy generally increase from left to right across a period? Multiple choice question. a. Electron repulsions decrease, making it harder to remove the outermost electron. b. Electron repulsions increase, making it easier to remove the outermost electron. c. The closer one gets to a noble gas the more likely an element is to gain an electron. d. Effective nuclear charge increases and the outermost electron becomes harder to remove.

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

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. Multiple choice question. a. farther away from; more b. closer to; less c. closer to; more d. farther away from; less

d. farther away from; less

When an electron is removed from an atom the atomic radius decreases and when an electron is added the atomic radius increases. This is due in large part to changes in _____.

electron-electron repulsions

Match each type of element correctly to its characteristic properties. metals nonmetals metalloids

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

Rank the following elements in order of increasing metallic character (from least metallic at the top of the list to most metallic at the bottom). Instructions n(7) Ga(31) Co(27) Ba(56)

n(7) Ga(31) Co(27) Ba(56)

Which electrons are removed first when forming cations of period 4 transition elements?

4s

Which of the following statements correctly describe atomic radii? Select all that apply. Multiple select question. a. Atomic radii of main group elements decrease from Group 1A to Group 8A. b. Atomic radii decrease as the effective nuclear charge (Zeff) decreases. c. Atomic radii generally increase as n increases.

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+

Match the trends in ionization energies correctly. Instructions IE decreases IE increases down a group. from left to right across a period.

IE decreases: down a group. IE increases: from left to right across a period.

Which of the following statements correctly describe the trends in ionic size? Select all that apply.

Ionic size increases down a group on the periodic table. Anions are larger than their parent atom.