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S block elements

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Colorless ions Silvery colored when neutral Important biological functions

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F block elements

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Mostly have 3+ charges Pale colored in solution No important biological functions

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D block elements

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Usually 2+ or 3+ charges Intermediate color intensity in solution Most have positive biological functions as ions or complexes

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P block elements

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Contains cations and anions Colorless in solution

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Covalent radius

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1/2 the internuclear distance 1/2 the length of the covalent bond For a bond between 2 identical atoms

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Ionic radii of cations/anions

answer

The sums of the ionic radii

question

Van der waals radius

answer

1/2 the internuclear distance to the nearest Cl nucleus in the next molecule

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Sizes of radii

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Cationic < covalent < anionic = van der waals Difference of 60pm between each type

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Horizontal trend of atomic radii

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Decrease moving from L to R More protons pull electrons closer, causing a smaller radius

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Vertical trend of atomic radii

answer

Increase from top to bottom

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Scandide contraction

answer

Nonexpansion in period 4 Involves Al and Ga

question

Lanthanide contraction

answer

Nonexpansion in period 6

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Bronsted-Lowry acid

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Proton donor (becomes conj base)

question

Bronsted-Lowry base

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Proton acceptor (becomes conj acid)

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Amphiprotic

answer

Something that is both basic and acidic, but not strongly either

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6 strong acids

answer

1. HCl 2. HBr 3. HI 4. H2SO4 5. HClO4 6. HNO3

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Lower pKa

answer

Lower pH = MORE ACIDIC

question

Lower pKb

answer

Higher pH = MORE BASIC

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Strong acids produce?

answer

A weak conjugate base

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Weak acids produce?

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A strong conjugate base

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Nonacidic cations

answer

pKa > 14 Do not alter pH of solution

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Feebly acidic cations

answer

pKa between 11.5 and 14

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Weakly acidic cations

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pKa between 6 and 11.5

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Moderately acidic cations

answer

pKa between 1 and 6

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Strongly acidic cations

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pKa between -4 and 1 React violently and exothermically

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Very strongly acidic cations

answer

pKa < -4 Cannot actually exist in solution

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Acidity of a metal cation solution depends on?

answer

1. charge 2. radius 3. electronegativity

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Charge and acidity of metal cations

answer

As charge increases, acidity strongly increases due to increased interaction and more dissociation

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Radius and acidity of metal cations

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As radius increases, acidity decreases Increased stability of cation leads to less interactions

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Electronegativity and acidity of metal cations

answer

As electronegativity increases, acidity increases

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Hydration enthalpies of cations are affected by?

answer

1. charge 2. radius 3. electronegativity

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Charge and hydration enthalpies of cations

answer

As charge increases, deltaH gets more negative, acidity increases Charge has the biggest effect on deltaH!!!!!!!!!

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Radius and hydration enthalpies of metal cations

answer

As radius increases, deltaH gets less negative, acidity decreases`

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Electronegativity and hydration enthalpies of metal cations

answer

As electronegativity increases, deltaH gets more negative and acidity increases

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Maximum coordination number

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The max number of atoms bound to the central atom Depends on the size of the atoms bound to the central atom Generally increases moving down the periodic table

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Maximum coordination number for period 2

answer

4

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Maximum coordination number for periods 3 and 4

answer

6

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Maximum coordination number for periods 5 and 6

answer

> 6, usually 8

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When maximum coordination number is met?

answer

No reaction will occur in water due to steric hindrance

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Why do some elements have lower than normal coordination numbers?

answer

Ions in periods 5 and 6 (Ag+, Sn3+, Hg+, Au+) attach as few as 2 water molecules The polarizing power of the cationic charge is concentrated on fewer water molecules Each water molecule is more polarized, leading to HIGHER THAN EXPECTED ACIDITY.

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Henderson-Hasselbach equation

answer

pH = pKa + log [conj base]/[conj acid]

question

Equivalence point

answer

When moles of acid = moles of base In titration NOT IMPORTANT

question

Half-equivalence point

answer

When concentrations of acid and base are equal pH at this point = pH at right boundary = pKa1

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Predominance diagram

answer

Anions on R Cations on L

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Predominance diagrams and predicting reactions

answer

If there is no overlap, the reactants cannot coexist as predominant forms in the same pH, so a reaction will occur (proton transferred L to R) If there is overlap, the reactants can coexist so there will be NO REACTION

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Nomenclature of group 16 hydrides

answer

H2S: hydrogen sulfide H2Se: hydrogen selenide H2Te: hydrogen telluride

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Nomenclature of group 14 hydrides

answer

End in "-ane" Plumbane, stannane, germane, silane Formulas written w/ H+ last to show that they are not predominantly acidic

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Nomenclature of group 15 hydrides

answer

End in "-ine" Bismuthine, arsine, phosphine Formulas written with H+ last to show that they are not predominantly acidic

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Nomenclature of group 17: hydrogen halides

answer

In solution, they undergo acid dissociation and are named as hydrohalic acids

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Predominance diagram of a nonacidic cation

answer

Cation is predominant at all pH values

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Predominance diagram of a feebly acidic cation

answer

Precipitates hydroxides from 1M solutions at pH > 11.5-14

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Predominance diagram of a weakly acidic cation

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Precipitates metal hydroxides at pH 6-11.5 (neutral to slightly basic

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Predominance diagram of a moderately acidic cation

answer

Cation is predominant in solution at pH 1-6, ppt forms if the solution is not kept acidic

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Predominance diagram of a strongly acidic cation

answer

Cation is predominant in solution at pH -4 to 1 At most practical pH values there is a metal hydroxide ppt

question

Predominance diagram of a very strongly acidic cation

answer

Cannot exist in water because it is impossible to have a pH that low in water

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As concentration decreases?

answer

The range of soluble species increases!!!

question

Hydrated anions

answer

A H bond forms between a H on the water and the metal anion, ripping the H off the water molecule and producing OH- to form a basic solution

question

Nonbasic anions

answer

pKb > 14 No detectable basicity Cl-, Br-, I- No tendency to combine with H+ ions in solution So much less basic than water that they cannot compete with water for H+ ions

question

Feebly basic anions

answer

pKb values 11.5-14 No examples

question

Weakly basic anions

answer

pKb values 6-11.5 Includes F-

question

Moderately basic anions

answer

pKb values 1-6 Te2-

question

Strongly basic anions

answer

pKb values -4 to 1 Se2-, S2-

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Very strongly basic anions

answer

pKb < -4 React irreversibly with water O2- + H2O = 2OH-

question

Factors that affect basicity of anions

answer

1. charge 2. radius

question

Charge and basicity of anions

answer

As the charge gets larger and more negative, the basicity increases Basicity increases moving L to R across a period

question

Radius and basicity of anions

answer

As radius increases, basicity decreases Basicity decreases moving down a group

question

Periodic trends in basicity

answer

The further up and into the periodic table an element is, the more reactive its ion is (as long as charge is increasing)

question

Reactions between strong acids and bases

answer

React to give species with overlapping ranges closer to the center of the predominance diagram

Inorganic Chemistry Exam 1, Chapters 1 and 2 – Flashcards

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