Quantum model, Bonds, Arranging Atoms in Molecules, Electronegativity, Molecule Polarity and Intermolecular forces

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Last updated 8:34 AM on 6/4/26
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18 Terms

1
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What is the Quantum Model?

-3d model of atoms

-Electrons are arranged in areas of probability 95% of time

-Electrons behave like waves

<p><span>-3d model of atoms</span></p><p><span>-Electrons are arranged in areas of probability 95% of time</span></p><p><span>-Electrons behave like waves</span></p>
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<p>What is the <strong>Electron Configuration</strong> of <span><span>Br</span></span><sup>-</sup> ?</p>

What is the Electron Configuration of Br- ?

1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6

<p><span><span>1s</span></span><sup>2</sup><span><span> 2s</span></span><sup>2</sup><span><span> 2p</span></span><sup>6</sup><span><span> 3s</span></span><sup>2</sup><span><span> 3p</span></span><sup>6</sup><span><span> 4s</span></span><sup>2</sup><span><span> 3d</span></span><sup>10</sup><span><span> 4p</span></span><sup>6</sup></p>
3
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How is the first full orbit of each type represented in the Quantum Model?

1s²

2p6

3d10

4
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What is Metallic Bonding?

in pure metals, the protons in atoms attract electrons in nearby atoms

<p>in pure metals, the protons in atoms attract electrons in nearby atoms</p>
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What is Covalent Bonding?

-Non metal + Non metal

-Electronegativity difference < 1.7

-Shared electrons

<p>-Non metal + Non metal</p><p>-<strong>Electronegativity difference &lt; 1.7</strong></p><p><strong>-Shared electrons</strong></p>
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What is Ionic Bonding?

-Metal+non metal

-Occurs if Electronegativity is > 1.7

-Transfer electrons

<p>-Metal+non metal </p><p>-Occurs if <strong>Electronegativity is &gt; 1.7</strong></p><p><strong>-Transfer electrons</strong></p>
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What is the Octet Rule?

All atoms want a full outer shell of 8 electrons (except H wants 2)

8
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What is Electronegativity(E.N)?

An atom’s ability to attract outer electrons

*Electrons shared if small difference

*Electrons transfer if big difference

<p>An atom’s <strong>ability </strong>to <strong>attract outer electrons</strong></p><p><strong>*</strong>Electrons <strong>shared </strong>if <strong>small difference</strong></p><p><strong>*</strong>Electrons <strong>transfer </strong>if <strong>big difference</strong></p>
9
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VSEPR theory

Valence Shell Electron Pair Repulsion

-Electrons repel and determine molecule shape

<p><strong>V</strong>alence <strong>S</strong>hell <strong>E</strong>lectron <strong>P</strong>air <strong>R</strong>epulsion</p><p>-Electrons repel and determine molecule shape</p>
10
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What is Molecular Polarity?

Uneven distribution of electrical charge across a molecule, creating a positive and a negative "pole."

<p><strong>Uneven distribution of electrical charge</strong> across a molecule, creating a positive and a negative "pole."</p>
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What does Molecular Polarity depend on?

-Molecule shape

-Electronegativity(E.N) difference(δ) between bonds

If δ > 0.4 AND δ ≤ 1.8 = Polar

<p>-Molecule shape</p><p>-Electronegativity(E.N) difference(δ) between bonds</p><p></p><p>If <strong>δ &gt; 0.4</strong> AND <strong>δ ≤ 1.8 </strong>= <strong>Polar</strong></p>
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What are Intermolecular Forces?

-Forces of attraction between molecules

-Evidence shown in boiling point, melting point and surface tension

-Strength increases with Molecule Size

<p>-Forces of <strong>attraction between molecules</strong></p><p>-<strong>Evidence </strong>shown in <strong>boiling point, melting point and surface tension</strong></p><p>-<strong>Strength increases</strong> with <strong>Molecule Size</strong></p>
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What are the types of Intermolecular Forces in order of descending strength?

| Hydrogen Bonds

| Dipole Force

| London Force

*

<p>| Hydrogen Bonds</p><p>| Dipole Force</p><p>| London Force</p><p>*</p>
14
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Characteristics of London Force

-Caused by a temporary uneven distribution of elements

-Weakest intermolecular force

<p>-Caused by a temporary uneven distribution of elements</p><p>-Weakest intermolecular force</p>
15
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What Intermolecular Forces would require the highest temperature to break apart?

Hydrogen bonds

16
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Characteristics of Dipole Force

-Attractive forces between polar molecules

-Stronger than London Force

<p>-Attractive forces between <strong>polar molecules</strong></p><p><strong>-</strong>Stronger than London Force</p>
17
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Characteristics of Hydrogen Bonds

-Occur in molecules with H and either N, O or F

-Strongest intermolecular force

*Responsible for water’s high boiling point and shape of snowflakes

<p>-Occur in molecules with <strong>H </strong>and <strong>either</strong> <strong>N</strong>, <strong>O</strong> or <strong>F</strong></p><p>-Strongest intermolecular force</p><p>*<strong>Responsible</strong> for <strong>water’s high boiling point</strong> and <strong>shape of snowflakes</strong></p>
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Why are Hydrogen Bonds the strongest type of Intermolecular Force?

Because, N, O, F have only 2 shells so H gets the closer to the nucleus making it harder to break the bonds.