Question

elements in the same column:

• have similar ______ _____________
• have same number of _____________ __________________
• have similar _____________ _____________
• electron distribution for ne: _______________________________

kr: _______________________________________
noble gases:

• have __________ outer ________ __________
• have ____ valence _____________
• are _______________

using periodic table to find electron distributions:
\s\ section
e level = period #
\d\ section
e level = period # - 1
\p\ section
e level = period #
\f\ section
e level = period # - 2
noble gas distributions - find noble gas on end of row before the element and put its symbol in brackets.
use diagonal rule to write electron distribution of sn (atomic no. 50):
_______________________________
use noble gas distribution to write electron distribution of sn:
___________________
the chemistry quiz
cr1. cr2. 1. 2.

Explanation:

Part 1: Elements in the same column

Elements in the same column (group) of the periodic table have similar chemical properties, the same number of valence electrons, similar reactivity patterns, and follow trends in electron distribution. For noble gases (Ne, Kr), their electron distributions are stable (full valence shells).

• Similar: chemical properties
• Same number of: valence electrons
• Similar: reactivity (or chemical behavior)
• Electron distribution:
• Ne: $1s^2 2s^2 2p^6$ (full $n=2$ shell)
• Kr: $1s^2 2s^2 2p^6 3s^2 3p^6 3d^{10} 4s^2 4p^6$ (full $n=4$ shell)

Part 2: Noble Gases

Noble gases have full outer electron shells, 8 valence electrons (except He, which has 2), and are chemically inert (unreactive) because their electron configuration is stable.

• have: full outer electron shells
• have: 8 valence electrons (He has 2)
• are: inert (unreactive)

Part 3: Electron Distribution of Sn (Atomic No. 50)

Step 1: Diagonal Rule (Aufbau Principle)

The diagonal rule dictates electron filling order: $1s \to 2s \to 2p \to 3s \to 3p \to 4s \to 3d \to 4p \to 5s \to 4d \to 5p \to \dots$

• $1s$: 2 electrons
• $2s$: 2 electrons (total: 4)
• $2p$: 6 electrons (total: 10)
• $3s$: 2 electrons (total: 12)
• $3p$: 6 electrons (total: 18)
• $4s$: 2 electrons (total: 20)
• $3d$: 10 electrons (total: 30)
• $4p$: 6 electrons (total: 36)
• $5s$: 2 electrons (total: 38)
• $4d$: 10 electrons (total: 48)
• $5p$: 2 electrons (total: 50, matching Sn’s atomic number)

Thus, the electron distribution via the diagonal rule is:
$$1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^{10} 4p^6 5s^2 4d^{10} 5p^2$$

Step 2: Noble Gas Distribution

Noble gas distribution uses the nearest noble gas (Kr, atomic no. 36) as a shortcut.

• Kr’s electron configuration: $1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^{10} 4p^6$ (or $[Kr]$)
• Sn has 50 – 36 = 14 more electrons. These fill $5s^2$, $4d^{10}$, and $5p^2$.

Thus, the noble gas distribution is:
$$[Kr] 5s^2 4d^{10} 5p^2$$

Final Answers

1. Elements in same column:

• Similar: $\boldsymbol{\text{chemical properties}}$
• Same number of: $\boldsymbol{\text{valence electrons}}$
• Similar: $\boldsymbol{\text{reactivity (chemical behavior)}}$
• Ne: $\boldsymbol{1s^2 2s^2 2p^6}$; Kr: $\boldsymbol{1s^2 2s^2 2p^6 3s^2 3p^6 3d^{10} 4s^2 4p^6}$

1. Noble Gases:

• have: $\boldsymbol{\text{full}}$ outer $\boldsymbol{\text{electron shells}}$
• have: $\boldsymbol{8}$ valence $\boldsymbol{\text{electrons}}$
• are: $\boldsymbol{\text{inert (unreactive)}}$

1. Sn electron distribution:

• Diagonal rule: $\boldsymbol{1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^{10} 4p^6 5s^2 4d^{10} 5p^2}$
• Noble gas: $\boldsymbol{[Kr] 5s^2 4d^{10} 5p^2}$

Answer:

Noble gases have full outer electron shells, 8 valence electrons (except He, which has 2), and are chemically inert (unreactive) because their electron configuration is stable.

• have: full outer electron shells
• have: 8 valence electrons (He has 2)
• are: inert (unreactive)

Part 3: Electron Distribution of Sn (Atomic No. 50)

Step 1: Diagonal Rule (Aufbau Principle)

The diagonal rule dictates electron filling order: $1s \to 2s \to 2p \to 3s \to 3p \to 4s \to 3d \to 4p \to 5s \to 4d \to 5p \to \dots$

• $1s$: 2 electrons
• $2s$: 2 electrons (total: 4)
• $2p$: 6 electrons (total: 10)
• $3s$: 2 electrons (total: 12)
• $3p$: 6 electrons (total: 18)
• $4s$: 2 electrons (total: 20)
• $3d$: 10 electrons (total: 30)
• $4p$: 6 electrons (total: 36)
• $5s$: 2 electrons (total: 38)
• $4d$: 10 electrons (total: 48)
• $5p$: 2 electrons (total: 50, matching Sn’s atomic number)

Thus, the electron distribution via the diagonal rule is:
$$1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^{10} 4p^6 5s^2 4d^{10} 5p^2$$

Step 2: Noble Gas Distribution

Noble gas distribution uses the nearest noble gas (Kr, atomic no. 36) as a shortcut.

• Kr’s electron configuration: $1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^{10} 4p^6$ (or $[Kr]$)
• Sn has 50 – 36 = 14 more electrons. These fill $5s^2$, $4d^{10}$, and $5p^2$.

Thus, the noble gas distribution is:
$$[Kr] 5s^2 4d^{10} 5p^2$$

Final Answers

1. Elements in same column:

• Similar: $\boldsymbol{\text{chemical properties}}$
• Same number of: $\boldsymbol{\text{valence electrons}}$
• Similar: $\boldsymbol{\text{reactivity (chemical behavior)}}$
• Ne: $\boldsymbol{1s^2 2s^2 2p^6}$; Kr: $\boldsymbol{1s^2 2s^2 2p^6 3s^2 3p^6 3d^{10} 4s^2 4p^6}$

1. Noble Gases:

• have: $\boldsymbol{\text{full}}$ outer $\boldsymbol{\text{electron shells}}$
• have: $\boldsymbol{8}$ valence $\boldsymbol{\text{electrons}}$
• are: $\boldsymbol{\text{inert (unreactive)}}$

1. Sn electron distribution:

• Diagonal rule: $\boldsymbol{1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^{10} 4p^6 5s^2 4d^{10} 5p^2}$
• Noble gas: $\boldsymbol{[Kr] 5s^2 4d^{10} 5p^2}$