State whether each of the following properties of the representative elements generally increase

State whether each of the following properties of the...

Key Concepts

Acidity of Oxides

The acidity of oxides is a measure of how an oxide reacts with water or bases to produce acidic solutions. Generally, oxides become more acidic from left to right across a period as elements become more electronegative, while down a group, the acidic nature of the oxides typically decreases, reflecting an increase in metallic character.

Ionization Energy

Ionization energy is the amount of energy required to remove an electron from an atom or ion in the gaseous state. This property generally increases across a period as the effective nuclear charge strengthens the hold on electrons, and decreases down a group as increased electron shielding in larger atoms makes it easier to remove an electron.

Periodic Trends

Periodic trends refer to the general patterns observed in the physical and chemical properties of elements as one moves across a period or down a group in the periodic table. These trends are influenced by factors such as effective nuclear charge, electron shielding, and subshell filling, which collectively determine changes in atomic and electronic structure.

Metallic Character

Metallic character describes an element's ability to lose electrons and exhibit typical metallic properties such as malleability and conductivity. Across a period, metallic character generally decreases as elements become less metallic and more nonmetallic, while down a group it typically increases due to the added electron shells and shielding effect.

Atomic Size

Atomic size, or atomic radius, refers to the distance from the nucleus to the outermost electron shell. Moving from left to right across a period, atomic size usually decreases because of the increasing effective nuclear charge that pulls electrons closer to the nucleus, whereas, moving down a group, atomic size increases due to the addition of electron shells.

Transcript

00:01 If you want to make some generalizations about certain characteristics like the ones we're given, it helps by examining the trends on the periodic table.

00:13 So we'll look at it from left to right as well as from top to bottom.

00:20 So if we start with metallic character of an element, we can start out by recognizing that the metals are generally found on the left side of the periodic table.

00:29 And on the right side are the non -metal.

00:31 So they have less conductive ability for electrons, and they're generally less lustrous than they're found in the gas phase naturally on the right side, whereas on the left side, they are better at conducting electricity and have more metallic characteristics.

00:47 So as we go from the left to the right, metallic character will decrease.

00:54 And if we look from top to bottom, one way we can measure metallic character is by recognizing that elements that are, more likely to give up their electrons in a flow of electricity are going to be more metallic.

01:08 So because francium at the very bottom is less attracted to its valence electrons, it's probably going to have a better flow of electricity than hydrogen, which will hold onto its electron more closely.

01:24 So we can determine that metallic characteristic will increase going top to bottom.

01:32 For the atomic size, we know that going from left to right increases the effective nuclear charge because the number of protons is increasing.

01:42 So that means with a greater nuclear charge, there's going to be greater attraction on the electrons, and it's going to bring it closer to the center, thus decreasing the size.

01:53 So that means size goes left to right by decreasing...

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