Physical Properties
Q: What are the general physical properties of transition metals?
A: They are hard, have high density, high melting and boiling points, and good electrical/thermal conductivity.
Q: What type of ions do transition metals commonly form?
A: They commonly form positive ions (cations) with variable oxidation states.
Q: How does atomic radius change across a period?
A: Atomic radius decreases across a period due to increasing nuclear charge pulling electrons closer.
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Q: Why do transition metals have high melting points?
A: Due to strong metallic bonding caused by delocalized d-electrons.
Q: What is a characteristic oxidation state of Iron (Fe)?
A: Fe commonly shows +2 and +3 oxidation states
Q: How does ionization energy change down a group?
A: It decreases down a group because outer electrons are farther from the nucleus and experience more shielding.
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Q: Which transition metal is the best conductor of electricity?
A: Silver (Ag) is the best electrical conductor.
Q: Why do transition metals exhibit variable oxidation states?
A: Because their d-orbitals can lose different numbers of electrons.
Q: Why do transition metals show unique colors in compounds?
A: Due to d-d electron transitions in the presence of ligands.
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Q: What is the relationship between density and atomic structure in transition metals?
A: Higher atomic mass and compact atomic structure result in high density.
Q: What makes transition metals good catalysts?
A: They provide a surface for reactions and can change oxidation states to assist reactions.
Q: How does electronegativity change across the d-block?
A: Increases across the d-block due to increasing nuclear charge.
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Q: Explain why transition metals have a high tensile strength.
A: Strong metallic bonding and layered atomic structure prevent easy deformation.
Q: Describe the reaction of transition metals with acids.
A: They typically react slowly with acids, producing hydrogen gas and metal salts.
Q: Why do transition metals have higher melting points than alkali metals?
A: Due to stronger metallic bonding and delocalized d-electrons.
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