🔥Chemistry 1.6 -the Peridoic Table Flashcards by jessica gregory

How does Ionisation energy increase in the periodic table?

Upward diagonally, fluorine is the element with the highest I.E

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How does Electronegativity increase in the periodic table?

It increases diagonally up the periodic table, fluorine is the most electronegative element

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Where in the periodic table is the s block

Group 1 and 2

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Where In the periodic table is the d block

Transition metals

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Where in the periodic table is the p block?

3,4,5,6,7, 8 (inert gas)

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Where are cations and ionic compounds formed?

Why?

Formed in the S Block because electrons in this block are readily lost

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Why is covalencey usually found in the P block

Because group 3’s ionisation energy becomes too high allowing electron sharing to occur

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Where are anions in ionic compounds found in the periodic table?
Why?

In group 6&7 because the more electronegative elements can accept electrons readily to form the anions

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Name the trend in valency in the periodic table

Valency normally rises with the groups to a maximum of 4 and then decreases (8-group number) to one in group 7

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If an element had a low I.E what is it likely to be?

A metal in the lower left region of the table

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If an element has a high I.E what is it likely to be?

Non metal in the upper right of the table

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What are the elements found between those with High and low I.E called?
Give an example

Portion and semiconductor elements such as Silicon

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What is the oxidisation number of a group 1 and group 2 metal?

Group 1= +1

Group 2= +2

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What ions are found in the s block

Cations

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In a redox reaction are the s block elements oxidising or reducing agents

Reducing

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Name the melting temperature in group 1

Decreased down the group

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Describe the oxides in the s block

Basic

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Describe the melting temperature trend until the end of group 4

Increase across a period up until group 4 (carbon melts above 3500 etc)

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Name the ions in the p block (excluding group 8)

Anions

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Name the oxidisation number of group 6 and 7

Group 6 = -2

Group 7= -1

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In a redox reaction are group 6 and 7 reducing or oxidising agents?

Oxidising

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Describe the oxides in group 6/7

Acidic

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Describe the melting point in group 6 and 7

The melting point increases down the groups

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What type of element is in group 6/7

Non metal

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What kind of element is in the s block?

Metal

What determines the trend in salt solubility | Name 2 examples

The strength of the lattice in an ionic crystal, stronger the lattice the more insoluble the compound 1) In MgSO4 the Mg ion is much smaller than the SO4 ion so the ions can’t fit well together to form the strong lattice and MgSO4 is soluble 2) In BaSO4 the Ba ion is much bigger than Mg, the ions fit together well in the lattice and BaSO4 is insoluble in water

Name the solubility is group 1

All salts are soluble

Name the solubility of carbonates | For when X= group 1 or group 2

All insoluble

Name the solubility of sulfates (XSO4) | For when X= group 1 or group 2

Solubility decreases down the group, BaSO4 = insoluble

Name the solubility of X(OH)2 compounds | For when X= group 2 hydroxide

Solubility increase down the group e.g Mg(OH)2 is insoluble

If an element/compound looses electrons is it oxidised or reduced?

Oxidised

If an element gains electrons is it oxidised or reduced

Reduced

In the equation: Na + 0.5Cl(2) —> Na+ + Cl- what has been oxidised and what has been reduced?

Sodium (Na) is oxidised as it lost an electron | Chlorine has been reduced as it has gained an electron

What is the oxidisation number of all elements on their own

What is the oxidisation number of hydrogen?

What is the oxidisation number of oxygen? | What is the exception?

-2 normally, -1 in H2O2

What is the oxidisation number of an element bound to itself?

What should all oxidisation numbers of elements in a compound or ion total to?

Add up to 0 or the charge of the ion e.g in MnO4- Ox4 = -8 This means that the Oxidisation number of Mn= +7

The S block elements: | Name the key sentence regarding S block elements

All reactive, electropositive (low electronegativity) metals forming cations with oxidisation number of 1 and 2 respectively

The S block elements: How are S block oxides formed? Give an example

Formed with oxygen/air | E.g Ca + 0.5O2 —> CaO

The S block elements: | How do you produce hydrogen (H2) with a group 1/2 metal?

Add water to the metal e.g | Na + H20 —> NaOH + 0.5H2

The S block elements: | How do group 1/2 metals react with acids?

A salt is formed and the elements act as reducing agents, donating electrons to reduce the acid or water to hydrogen and being themselves oxidised Mg + 2HCL —> MgCl2 + H2

The S block elements: | Trend in reactivity in group 1/2 metals?

Reactivity increases down the group, group 1 elements are more reactive than group 2 E.g Li reacts slowly with water whereas K reacts violently

The S block elements: | Describe how S block metals react with acids

Vigorously

The S block elements: | Which reacts more quickly with water Mg or Ba

Barium is faster

The S block elements: | What do I mean when I say the S block oxides are all basic

They react with acids to give salts as in: | CaO + 2HCL —> CaCl2 + H2O

The S block elements: | What S block element inflames spontaneously

Caesium

The S block elements: | Name the hydroxide solubilitues between Mg and Ba

Hydroxide solubilities = rise from 0.01g dm-3 in Mg to 3.9g dm-3 in Ba

The S block elements: | Name the sulfate solubilities between Mg and Ba

Fall down the group from 330g dm-3 in Mg to 0.002g dm-3 in Ba

The S block elements: | Are all group 2 carbonates soluble or insoluble

Insoluble

The S block elements: | Are all S block nitrates soluble or insoluble?

Insoluble

The S block elements: | Describe the trend in group 2 hydroxides and carbonates thermal stability

Increases down the group, E.g magnesium carbonate decomposes at 400 degrees vs barium carbonate which decomposed at 1300 degrees

The S block elements: | Where are calcium phosphate minerals found?

Living bones and skeletons

The S block elements: | Name one place where the carbonates exist in huge amounts

in rocks such as chalk and limestone and

The halogens: | Name the important sentence to know about halogens

Reactive, electronegative element which typically form anions having oxidisation states or -1 meaning oxidisation is the normal reaction

The halogens: | Give an example of an equation forming anions

Na + 0.5Cl2 —-> Na+ + Cl-

The halogens: | Name the trend in anion formation in group 7

The tendency to form anions decrease down the group from fluorine to iodine with fluorine being the most electronegative element

The halogens: | Name the trend in melting temperatures of halogens

The melting temperature decreases down the group from gaseous fluorine to solid iodine

The halogens: | Why does the trend in melting temperature increase down the group?

there is increasing number of intermolecular forces holding the diatomic elements together in a liquid/solid

The halogens: | Why are there the most intermolecular forces in iodine?

-the intermolecular forces are greatest in iodine because increasing numbers of electrons in molecules contribute to the induced dipole-dipole forces

The halogens: | Name the trend of reactivity in group 7

decreases down the group

The halogens: | What happens in s displacement reaction?

The more reactive halogen will displace the less reactive halogen E.g Cl2 + 2NaBr —> Br2 + 2NaCl

The halogens: | Describe the trend in oxidising power down the group

The oxidising power decreases down the group, for example in the equation: Cl2 + 2NaBr —> Br2 + 2NaCl The chlorine oxidises bromine ion to bromine and itself being reduced to chloride

If the oxidisation number increase is the element oxidised or reduced?

The element is oxidised

If the oxidisation number decreases is the element oxidised or reduced?

Reduced

The halogens: | Name the general silver chloride reaction

Ag+(aq) + X- (aq) —> AgX(s)

``` The halogens: In a silver nitrate reaction name the following precipitates: Chloride Bromide Iodide ```

``` Chloride = white Bromide = pale cream Iodide = pale yellow ```

The halogens: | How does chlorine make water safe to drink?

It kills pathogenic bacteria and viruses and prevents the outbreak of serious diseases such as typhoid and cholera

The halogens: | How is chlorine added to water?

Commonly added as the gaseous element Cl2 and sets up the equilibrium: Cl2 + H20 —> HOCL +HCL

The halogens: | At what dose does chlorine have a beneficial role in water?

Below 1 part per million (ppm)

The halogens: | Where is fluoride normally added?

Water and toothpaste

The halogens: | Why is Fluorine beneficial?

It reduces tooth decay caused by cavity formation and is used to strengthen bones, reducing osteoporosis

The halogens: | How is fluorine added to water?

Added as fluorosilic acid, sodium fluoride or sodium fluorosilicate

The halogens: | Why is there opposition to fluoridating water?

On ethical grounds