Chapter 4:

Without reference to the periodic table, match each atom (number of electrons given) with its block designation (s-, p-, or d-block) on the periodic tables. Hint: Write out the electron configuration for each example. 15 electrons -> d-block 20 electrons -> s-block 43 electrons -> p-block

15 electrons -> p-block 20 electrons -> s-block 43 electrons -> d-block

Which type of electrons are best at shielding a 3p electron? 3d 3p 3s 2p 4p

2p bc Electrons in inner energy levels are best at shielding other electrons

Which elements are removed first when forming cations of period 4 transition elements? 3d 4d 3p 4s

4s

Noble gasses

All elements in this group have a valence electron config of n^2np^6

Halogens

All elements in this group have a valence electron config of ns^2np^5

Transition Metals

All elements in this group have incompletely filled d subshells.

Lanthanides and Actinides

All elements in this group have incompletely filled f subshells.

Which of the following groups contains elements that are chemically similar to each other because they have the same valence-electron config? Noble gases Transition metals Halogens Alkali metals

All except Transition metals

Match each type of ion with the correct description of its size relative to its parent atom. Cation Anion ___________________________________________ Smaller than its parent atom Larger than its percent atom

Cation -> Smaller than its parent atom Anion -> Larger than its percent atom

Match the group number from the periodic table with the correct name. Elements in Groups 1A - 7A Group 8A Elements in Groups 18 and 3B f- block transition elements ____________________________________________ transition metals noble gases lanthanides and actinides main group elements

Elements in Groups 1A - 7A -> main group elements Group 8A -> noble gases Elements in Groups 18 and 3B->transition metals f-block transition elements -> lanthanides and actinides

Ionization trends

IE decreases down a group and increases left to right.

Metallic Character

Increases left to right Decreases down a group

Atomic size

Increases left to right Decreases up a group

Atomic Radius

Increases left to right and down a group.

Order the following elements in terms of increasing effective nuclear charge (Zeff) Br Cs K As

K Ca As Br

Match each of the following element with the correct number of electrons lost or gained to form its most common ion. K -> loses 1 electron Cl -> gains 1 electron Mg -> gains 2 electrons S -> loses 2 electrons

K -> loses 1 electrons Cl -> gains 1 electrons Mg -> loses 2 electrons S -> gains 2 electrons

Based on their positions in the periodic table, match the elements that are most chemically similar. K Cs Mg Cl F Sr Ne Ar

K Cs Mg Sr F Cl Ne . Ar

which of the following ions are isoelectronic with Ar? Select all that apply. Br^- K^+ Cl^- Mg^2+ S^2-

K^+, Cl^-, S^2-

List the following elements in order of decreasing

Periodicity

The periodic table developed from the observation of ________________, which is the regular recurrence of the physical and chemical properties of the elements when they are arranged in order of increasing atomic mass.

Periodicity

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 config 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. Al is farther to the right in the periodic table and has a higher value for effective nuclear charge. Al will have a higher first ionization energy.

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.

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

S Br Se I

Isoelectronic

Same electrons

Repulsions between electrons in a many-electron atom results in a phenomenon known as ______________, which leads to the electrons "experiencing" a lower____________ nuclear charge.

Shielding, effective

Which of the following species are isoelectronic w/ each other? Ar Sr^2+ Mg^2+ Br^- Cd^2+

Sr^2+ Br^-

why do some elements (such as Li and Mg) exhibit diagonal relationships?

The cations of these elements have similar charge densities.

Covalent Radius

The covalent radius is half the distance between adjacent, identical nuclei that are connected by a chemical bond.

Metallic Radius

The metallic radius half the distance between the nuclei of two adjacent, identical metal atoms.

Mendeleev's original periodic table

The original Periodic table predicted the properties of elements that were not discovered until later. The original period table was developed by Dimitri Mandeleev The original periodic table had 66 elements.

Electron configuration for Sn^4+

[Kr]4d^10

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

a, b

Which of the following options correctly describes the shielding effects in a many-electron systems? a.) Shielding reduces the magnitude of the nuclear charge a given electron experiences. b.) Inner electrons are more effective at shielding outer electrons than electrons in the same level. c.) The shielding effect increases with an increasing number of electrons in a given sublevel. d.) Electrons in the same sublevel do not shield each other from the nucleus. e.) Shielding protects an electron so that it is harder to remove from the atom.

a, b, c

Which of the following statements correctly describes the changes that occur as we move from left to right across the periodic table? a.) Nuclear charge increases b.) The number of core electrons increases. c.) The nuclear charge felt by the outermost electrons decreases d.) The number of valence electrons increases for representative elements.

a, d

Which of the following statements describes/define ionization energy correctly? Select all that apply. a.) The ionization energy of an element is a measure of how easily it forms a cation. 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.) 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.

a, d

ionic radius

decreases for cations and anions from left to right across a period Decreases going up on a group.

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

decreases, increases

Elements such as Na and K are in the same ________________ of the periodic table. These elements have similar chemical properties because they have the same number of __________ electrons.

group, valence

As we move from left to right in the periodic table the effective nuclear charge (Zeff) __________ because the number of ___________ electrons remains the same while the actual nuclear charge increases.

increases, core

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

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 w/ a net ________________ charge.

ionization, cation, positive

Ions are most attracted to each other when their charges are ____________ and the distance between them is __________.

opposite, small