SSCE VCE Chemistry Chemical Elements: a. By referring to their electro

Question

a. By referring to their electron configurations, explain why metals in the first transition series of the periodic table typically have several different oxidation states while Group II metals have only one.

The transition metals are characterized by the presence of d-orbitals in addition to the s-orbitals. For example, the first transition series includes elements like Scandium (Sc) to Zinc (Zn), which have partially filled 3d subshells. This allows them to lose different numbers of electrons from both the 4s and 3d subshells, leading to multiple oxidation states. In contrast, Group II metals, such as the alkaline earth metals, have their s-orbitals filled, which means they can only lose their two outermost s electrons, resulting in a single oxidation state.

b. Predict the trend in the following properties of the second period elements, moving from lithium to fluorine, giving an explanation in support of each prediction.

Property          | Increases or decreases? | Explanation for predicted trend
-------------------|------------------------|--------------------------------
Atomic size        | decreases               | As we move across a period from left to right, the number of protons in the nucleus increases, which raises the effective nuclear charge. This increases the attraction between the nucleus and the outer electrons, thereby pulling them closer and reducing atomic size.
Electronegativity   | increases               | Moving from lithium to fluorine, the increasing nuclear charge enhances the attraction of the nucleus on the outer shell electrons, leading to a stronger tendency for these elements to attract electrons in a bond.

a. By referring to their electron configurations, explain why metals in the first transition series of the periodic table typically have several different oxidation states while Group II metals have only one - VCE - SSCE Chemistry - Question 6 - 2004 - Paper 1

Worked Solution & Example Answer:a. By referring to their electron configurations, explain why metals in the first transition series of the periodic table typically have several different oxidation states while Group II metals have only one - VCE - SSCE Chemistry - Question 6 - 2004 - Paper 1

By referring to their electron configurations, explain why metals in the first transition series of the periodic table typically have several different oxidation states while Group II metals have only one.

Predict the trend in the following properties of the second period elements, moving from lithium to fluorine, giving an explanation in support of each prediction. Property: Atomic size

Predict the trend in the following properties of the second period elements, moving from lithium to fluorine, giving an explanation in support of each prediction. Property: Electronegativity

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