Electronic Configuration and the Periodic Table readingAssignment

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 table. Hint: Write out the electron configuration for each example. 15 electrons 20 electrons 43 electrons

15 electrons: p block 20 electrons: s block 43 electrons: d block

Without using the periodic table, which of the following correctly represent the electron configuration of an element with 35 electrons? Select all that apply.

1s^2, 2s^2, 2p^6 3s^2, 3p^6, 4s^2, 3d^10, 4p^5 [Ar]4s^2, 3d^10, 4p^5

The nuclear charge an electron actually experiences is called the ____ nuclear charge (Z(subscript)eff). This charge is always ____ than the actual nuclear charge since in a many-electron system the electrons ____ each other from the nucleus.

Blank 1: effective Blank 2: less, lower, smaller, or weaker Blank 3: shield or screen

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

Blank 1: group, family, or column Blank 2: valence, outer, or outermost

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

Blank 1: shielding Blank 2: effective

The outermost electrons of an atom are called ____ electrons.

Blank 1: valence or valence shell

Match each group number from the periodic table with the correct name. Elements in Groups 1, 2, and 13-17 Group 18 Elements in Groups 3-11 f-block transition elements

Elements in Groups 1, 2, and 13-17: main group elements Group 18: noble gases Elements in Groups 3-11: transition metals f-block transition elements: lanthanides and actinides

Which is the highest occupied orbital for each of the following elements, based on their position on the periodic table? Instructions Mg As Co F 3s, 3d, 4p, 2p

Mg 3s As 4p Co 3d F 2p

What is the correct ground-state electron configuration for Mo?

[Kr]5s^1, 4d^5

Select the correct condensed electron configuration for the element S (Z = 16).

[Ne]3s^2 3p^4 Reason: Only noble gases are used as a reference in the condensed format, not other elements.

Which of the following groups contains elements that are chemically similar to each other because they have the same valence-electron configuration? Select all that apply. a. Alkali metals b. Transition metals c. Halogens d. Noble gases

a. Alkali metals c. Halogens d. Noble gases

Which of the following statements correctly describe different categories of electrons? Select all that apply. a. Ca has two valence electrons. b. Core electrons determine how atoms interact with each other. c. For main group elements, the group number is also the number of valence electrons. d. Valence electrons are the outermost electrons of an atom. e. All elements in group 17 react similarly because they all possess 5 valence electrons.

a. Ca has two valence electrons. c. For main group elements, the group number is also the number of valence electrons. d. Valence electrons are the outermost electrons of an atom.

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

a. Inner electrons are more effective at shielding outer electrons than electrons in the same level. c. Shielding reduces the magnitude of the nuclear charge a given electron experiences. e. The shielding effect increases with an increasing number of electrons in a given sublevel.

What characteristics do elements in the same group have in common? Select all that that apply. Multiple select question. a. Main group elements in the same group have the same number of valence electrons. b. Elements in the same group have the same electron configuration. c. Elements in the same group have similar chemical properties. d. Elements in the same group have similar physical properties.

a. Main group elements in the same group have the same number of valence electrons. c. Elements in the same group have similar chemical properties.

In a multi-electron atom, repulsions between electrons prevent valence electrons from "experiencing" the full positive charge of the nucleus. This repulsion is known as ______. a. shielding b. periodicity c. effective nuclear charge d. electron affinity

a. shielding

Which of the following statements correctly describe effective nuclear charge (Zeff)? Select all that apply. a. A lower Zeff is due to the loss of a proton from the nucleus. b. A lower Zeff makes a given electron easier to remove. c. Effective nuclear charge is only lowered by inner electrons. d. Effective nuclear charge is lowered by electron-electron repulsions.

b. A lower Zeff makes a given electron easier to remove. d. Effective nuclear charge is lowered by electron-electron repulsions.

Which of the following statements correctly describe the relationship between the electron configuration of an element and its position on the periodic table? Select all that apply. a. The highest occupied orbital for a Sr atom is a 4d orbital. b. Elements that are in the same group will have the same outer electron configuration. c. The highest occupied orbital for a Se atom is a 4p orbital. d. The electron configurations of transition metals follow a regular trend associated with their group numbers.

b. Elements that are in the same group will have the same outer electron configuration. c. The highest occupied orbital for a Se atom is a 4p orbital.

Which of the following statements correctly describe the relationship between the electron configuration of an element and its position on the periodic table? Select all that apply. a. The electron configurations of transition metals follow a regular trend associated with their group numbers. b. Elements that are in the same group will have the same outer electron configuration. c. The highest occupied orbital for a Se atom is a 4p orbital. d. The highest occupied orbital for a Sr atom is a 4d orbital.

b. Elements that are in the same group will have the same outer electron configuration. d. The highest occupied orbital for a Sr atom is a 4d orbital.

Which of the following elements exhibit an irregular filling pattern of the orbitals? Select all that apply. a. Cd b. Sr c. Cr d. Ag e. Cu

c. Cr d. Ag e. Cu

A condensed electron configuration includes the element symbol of the _____ gas that is _____ to the relevant element in square brackets, followed by the configuration of the energy level being filled. a. diatomic; prior b. diatomic; closest c. noble; prior d. noble; closest

c. noble; prior

Match each group of the periodic table with the type of electron configuration exhibited by elements in that group. Instructions completely filled p subshells incompletely filled d subshells incompletely filled f subshells - nobles gases (except He) - lanthanides and actinides - transition metals

completely filled p subshells: nobles gases (except He) incompletely filled d subshells: transition metals incompletely filled f subshells: lanthanides and actinides

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

d. 2p

Each of the following groups of elements have similar chemical properties, but for different reasons. Match each group with the correct reason for the similarities within the group. halogens noble gases transition metals lanthanides and actinides

halogens: All elements in this group have a valence-electron configuration of ns^2, np^5. noble gases: All elements in this group have a valence-electron configuration of ns^2, np^6. 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.