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Question
name: ____________ teacher: __________ q1 chemistry: u2l17.5 unit 2 mini review date: ____________ pre - work part 1: unit 2 review 1. for each of the following elements, write the full electron configuration, the orbital notation, and the noble gas configurations.
| element | full e⁻ configuration | orbital notation | noble gas config. |
|---|---|---|---|
| o | |||
| *s | |||
| co | |||
| na |
Step1: Determine electron - configuration rules
Use Aufbau principle, Pauli - exclusion principle and Hund's rule.
Step2: Find electron number of oxygen (O)
Oxygen has 8 electrons. Full electron configuration: $1s^{2}2s^{2}2p^{4}$.
Orbital notation:
$\frac{\uparrow\downarrow}{1s}$ $\frac{\uparrow\downarrow}{2s}$ $\frac{\uparrow\downarrow}{2p_x}$ $\frac{\uparrow}{2p_y}$ $\frac{\uparrow}{2p_z}$
Noble - gas configuration: $[He]2s^{2}2p^{4}$
Step3: Find electron number of sulfur (S)
Sulfur has 16 electrons. Full electron configuration: $1s^{2}2s^{2}2p^{6}3s^{2}3p^{4}$.
Orbital notation:
$\frac{\uparrow\downarrow}{1s}$ $\frac{\uparrow\downarrow}{2s}$ $\frac{\uparrow\downarrow}{2p_x}$ $\frac{\uparrow\downarrow}{2p_y}$ $\frac{\uparrow\downarrow}{2p_z}$ $\frac{\uparrow\downarrow}{3s}$ $\frac{\uparrow\downarrow}{3p_x}$ $\frac{\uparrow}{3p_y}$ $\frac{\uparrow}{3p_z}$
Noble - gas configuration: $[Ne]3s^{2}3p^{4}$
Step4: Find electron number of cobalt (Co)
Cobalt has 27 electrons. Full electron configuration: $1s^{2}2s^{2}2p^{6}3s^{2}3p^{6}4s^{2}3d^{7}$.
Orbital notation:
$\frac{\uparrow\downarrow}{1s}$ $\frac{\uparrow\downarrow}{2s}$ $\frac{\uparrow\downarrow}{2p_x}$ $\frac{\uparrow\downarrow}{2p_y}$ $\frac{\uparrow\downarrow}{2p_z}$ $\frac{\uparrow\downarrow}{3s}$ $\frac{\uparrow\downarrow}{3p_x}$ $\frac{\uparrow\downarrow}{3p_y}$ $\frac{\uparrow\downarrow}{3p_z}$ $\frac{\uparrow\downarrow}{4s}$
$\frac{\uparrow}{3d_{xy}}$ $\frac{\uparrow}{3d_{yz}}$ $\frac{\uparrow}{3d_{zx}}$ $\frac{\uparrow\downarrow}{3d_{x^{2}-y^{2}}}$ $\frac{\uparrow\downarrow}{3d_{z^{2}}}$
Noble - gas configuration: $[Ar]4s^{2}3d^{7}$
Step5: Find electron number of sodium (Na)
Sodium has 11 electrons. Full electron configuration: $1s^{2}2s^{2}2p^{6}3s^{1}$.
Orbital notation:
$\frac{\uparrow\downarrow}{1s}$ $\frac{\uparrow\downarrow}{2s}$ $\frac{\uparrow\downarrow}{2p_x}$ $\frac{\uparrow\downarrow}{2p_y}$ $\frac{\uparrow\downarrow}{2p_z}$ $\frac{\uparrow}{3s}$
Noble - gas configuration: $[Ne]3s^{1}$
| Element | Full $e^-$ configuration | Orbital notation | Noble gas config. |
|---|---|---|---|
| S | $1s^{2}2s^{2}2p^{6}3s^{2}3p^{4}$ | $\frac{\uparrow\downarrow}{1s}$ $\frac{\uparrow\downarrow}{2s}$ $\frac{\uparrow\downarrow}{2p_x}$ $\frac{\uparrow\downarrow}{2p_y}$ $\frac{\uparrow\downarrow}{2p_z}$ $\frac{\uparrow\downarrow}{3s}$ $\frac{\uparrow\downarrow}{3p_x}$ $\frac{\uparrow}{3p_y}$ $\frac{\uparrow}{3p_z}$ | $[Ne]3s^{2}3p^{4}$ |
| Co | $1s^{2}2s^{2}2p^{6}3s^{2}3p^{6}4s^{2}3d^{7}$ | $\frac{\uparrow\downarrow}{1s}$ $\frac{\uparrow\downarrow}{2s}$ $\frac{\uparrow\downarrow}{2p_x}$ $\frac{\uparrow\downarrow}{2p_y}$ $\frac{\uparrow\downarrow}{2p_z}$ $\frac{\uparrow\downarrow}{3s}$ $\frac{\uparrow\downarrow}{3p_x}$ $\frac{\uparrow\downarrow}{3p_y}$ $\frac{\uparrow\downarrow}{3p_z}$ $\frac{\uparrow\downarrow}{4s}$ $\frac{\uparrow}{3d_{xy}}$ $\frac{\uparrow}{3d_{yz}}$ $\frac{\uparrow}{3d_{zx}}$ $\frac{\uparrow\downarrow}{3d_{x^{2}-y^{2}}}$ $\frac{\uparrow\downarrow}{3d_{z^{2}}}$ | $[Ar]4s^{2}3d^{7}$ |
| Na | $1s^{2}2s^{2}2p^{6}3s^{1}$ | $\frac{\uparrow\downarrow}{1s}$ $\frac{\uparrow\downarrow}{2s}$ $\frac{\uparrow\downarrow}{2p_x}$ $\frac{\uparrow\downarrow}{2p_y}$ $\frac{\uparrow\downarrow}{2p_z}$ $\frac{\uparrow}{3s}$ | $[Ne]3s^{1}$ |
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Step1: Determine electron - configuration rules
Use Aufbau principle, Pauli - exclusion principle and Hund's rule.
Step2: Find electron number of oxygen (O)
Oxygen has 8 electrons. Full electron configuration: $1s^{2}2s^{2}2p^{4}$.
Orbital notation:
$\frac{\uparrow\downarrow}{1s}$ $\frac{\uparrow\downarrow}{2s}$ $\frac{\uparrow\downarrow}{2p_x}$ $\frac{\uparrow}{2p_y}$ $\frac{\uparrow}{2p_z}$
Noble - gas configuration: $[He]2s^{2}2p^{4}$
Step3: Find electron number of sulfur (S)
Sulfur has 16 electrons. Full electron configuration: $1s^{2}2s^{2}2p^{6}3s^{2}3p^{4}$.
Orbital notation:
$\frac{\uparrow\downarrow}{1s}$ $\frac{\uparrow\downarrow}{2s}$ $\frac{\uparrow\downarrow}{2p_x}$ $\frac{\uparrow\downarrow}{2p_y}$ $\frac{\uparrow\downarrow}{2p_z}$ $\frac{\uparrow\downarrow}{3s}$ $\frac{\uparrow\downarrow}{3p_x}$ $\frac{\uparrow}{3p_y}$ $\frac{\uparrow}{3p_z}$
Noble - gas configuration: $[Ne]3s^{2}3p^{4}$
Step4: Find electron number of cobalt (Co)
Cobalt has 27 electrons. Full electron configuration: $1s^{2}2s^{2}2p^{6}3s^{2}3p^{6}4s^{2}3d^{7}$.
Orbital notation:
$\frac{\uparrow\downarrow}{1s}$ $\frac{\uparrow\downarrow}{2s}$ $\frac{\uparrow\downarrow}{2p_x}$ $\frac{\uparrow\downarrow}{2p_y}$ $\frac{\uparrow\downarrow}{2p_z}$ $\frac{\uparrow\downarrow}{3s}$ $\frac{\uparrow\downarrow}{3p_x}$ $\frac{\uparrow\downarrow}{3p_y}$ $\frac{\uparrow\downarrow}{3p_z}$ $\frac{\uparrow\downarrow}{4s}$
$\frac{\uparrow}{3d_{xy}}$ $\frac{\uparrow}{3d_{yz}}$ $\frac{\uparrow}{3d_{zx}}$ $\frac{\uparrow\downarrow}{3d_{x^{2}-y^{2}}}$ $\frac{\uparrow\downarrow}{3d_{z^{2}}}$
Noble - gas configuration: $[Ar]4s^{2}3d^{7}$
Step5: Find electron number of sodium (Na)
Sodium has 11 electrons. Full electron configuration: $1s^{2}2s^{2}2p^{6}3s^{1}$.
Orbital notation:
$\frac{\uparrow\downarrow}{1s}$ $\frac{\uparrow\downarrow}{2s}$ $\frac{\uparrow\downarrow}{2p_x}$ $\frac{\uparrow\downarrow}{2p_y}$ $\frac{\uparrow\downarrow}{2p_z}$ $\frac{\uparrow}{3s}$
Noble - gas configuration: $[Ne]3s^{1}$
| Element | Full $e^-$ configuration | Orbital notation | Noble gas config. |
|---|---|---|---|
| S | $1s^{2}2s^{2}2p^{6}3s^{2}3p^{4}$ | $\frac{\uparrow\downarrow}{1s}$ $\frac{\uparrow\downarrow}{2s}$ $\frac{\uparrow\downarrow}{2p_x}$ $\frac{\uparrow\downarrow}{2p_y}$ $\frac{\uparrow\downarrow}{2p_z}$ $\frac{\uparrow\downarrow}{3s}$ $\frac{\uparrow\downarrow}{3p_x}$ $\frac{\uparrow}{3p_y}$ $\frac{\uparrow}{3p_z}$ | $[Ne]3s^{2}3p^{4}$ |
| Co | $1s^{2}2s^{2}2p^{6}3s^{2}3p^{6}4s^{2}3d^{7}$ | $\frac{\uparrow\downarrow}{1s}$ $\frac{\uparrow\downarrow}{2s}$ $\frac{\uparrow\downarrow}{2p_x}$ $\frac{\uparrow\downarrow}{2p_y}$ $\frac{\uparrow\downarrow}{2p_z}$ $\frac{\uparrow\downarrow}{3s}$ $\frac{\uparrow\downarrow}{3p_x}$ $\frac{\uparrow\downarrow}{3p_y}$ $\frac{\uparrow\downarrow}{3p_z}$ $\frac{\uparrow\downarrow}{4s}$ $\frac{\uparrow}{3d_{xy}}$ $\frac{\uparrow}{3d_{yz}}$ $\frac{\uparrow}{3d_{zx}}$ $\frac{\uparrow\downarrow}{3d_{x^{2}-y^{2}}}$ $\frac{\uparrow\downarrow}{3d_{z^{2}}}$ | $[Ar]4s^{2}3d^{7}$ |
| Na | $1s^{2}2s^{2}2p^{6}3s^{1}$ | $\frac{\uparrow\downarrow}{1s}$ $\frac{\uparrow\downarrow}{2s}$ $\frac{\uparrow\downarrow}{2p_x}$ $\frac{\uparrow\downarrow}{2p_y}$ $\frac{\uparrow\downarrow}{2p_z}$ $\frac{\uparrow}{3s}$ | $[Ne]3s^{1}$ |