Use the periodic table to determine each quantity. b. the number of 3d electrons in Cu d. the number of 4d electrons in Zr

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Step 1: Locate Copper (Cu) on the periodic table. Copper is in the 4th period and 11th group (or 1B in older notation).

Step 2: Identify the electron configuration of Copper. The electron configuration of Copper is [Ar] 4s2 3d9. However, Copper is one of the exceptions to the electron configuration rule. To stabilize the atom, one electron from the 4s orbital is moved to the 3d orbital, making the electron configuration [Ar] 4s1 3d10.

Step 3: Identify the number of 3d electrons. From the electron configuration, we can see that there are 10 electrons in the 3d orbital.

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Electron Configuration

Electron configuration describes the distribution of electrons in an atom's orbitals. For transition metals like copper (Cu), the electron configuration is crucial for understanding how many electrons occupy the 3d subshell. Copper has an atomic number of 29, leading to a configuration of [Ar] 3d10 4s1, indicating it has 10 electrons in the 3d subshell.

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Electron Configuration Example

Transition Metals

Transition metals are elements found in the d-block of the periodic table, characterized by their ability to form variable oxidation states and colored compounds. They typically have partially filled d orbitals, which play a significant role in their chemical properties. Understanding the behavior of transition metals, such as copper, is essential for determining the number of d electrons.

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Transition Metals

Periodic Table Trends

The periodic table organizes elements based on their atomic number and electron configurations, revealing trends in properties such as electronegativity, ionization energy, and atomic radius. By analyzing the position of copper in the periodic table, one can infer its electron configuration and the number of electrons in specific subshells, including the 3d subshell.

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