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Periodic Table, Group 2 & The Halogens QP 1

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Periodic Table, Group 2 & The Halogens QP 1

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Periodic Table, Group 2 & The Halogens QP 2

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Periodic Table, Group 2 & The Halogens QP 2

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Periodic Table, Group 2 & The Halogens QP 3

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Periodic Table, Group 2 & The Halogens QP 3

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Periodic Table, Group 2 & The Halogens QP 4

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Periodic Table, Group 2 & The Halogens QP 4

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Periodic Table Ionisation Energy
Successive ionisation energies apply to the removal of electrons after the first ionisation energy. The nth ionisation energy is:​

Ionisation energy is a measure of the energy required to completely remove an electron from an atom of an element to form an ion.

First ionisation energy is the energy required to remove one electron from each atom in one mole of the gaseous element to form one mole of gaseous 1+ ions.

Successive ionisation energies provide evidence for the shell structure of atoms.

Within each shell successive ionisation energies increase, as there is less electron repulsion

Between shells, there are big jumps in ionisation energies, as the electron is removed from a shell closer to the nucleus

Factors affecting ionisation energies:

Atomic radii- The larger the atomic radius, the further away the outer electrons are held from the nucleus, and the smaller the nuclear attraction.

Nuclear charge- The greater the nuclear charge, the greater the attractive force on the outer electrons.

Shielding- electrons repel each other due to their negative charge. The greater the number of inner shells of electrons, the greater the repulsion of the outer shell of electrons.

The greater the attraction, the harder it is to remove an electron. Therefore, the ionisation energy will be larger.

Atomic radii show periodicity. Across a period, the radius decreases while down a group, the radius increases.

Ionisation energy increases across a period, as nuclear charge increases, but shielding stays the same

In the Periodic Table, elements are arranged in order of increasing atomic number

Elements can be grouped into periods (horizontal rows) and groups (vertical columns)

Groups contain elements with similar physical and chemical properties, as they have the same number of outer shell electrons

Periodicity is a regularly repeating pattern of atomic, physical, and chemical properties with increasing atomic number

The Periodic Table can be split into s-, p-, d-, and f- blocks. Which is determined by which orbital the highest energy electron is in

​Giant Covalent Structures

Giant covalent lattices consist of billions of atoms held together by a network of strong covalent bonds.

Carbon forms three types of giant covalent structures: graphite, graphene and diamond.

In diamond, each carbon atom is bonded to four other carbon atoms

This makes it very strong, with an incredibly high melting point, hardness, insolubility. It is an electrical insulator because all the outer shell electrons are being used in covalent bonds, so there are no mobile charge carriers

Metallic Bonding Period 2 & 3
Across the period, the atomic radius decreases as effective nuclear charge increases and there is no increase in shielding

Across Period 2, two electrons fill the 2s sub-shell before six electrons will fill the 2p sub-shell

Across Period 3, two electrons will fill the 3s sub-shell before six electrons will fill the 3p sub-shell

Across Period 2 and Period 3, the trend in meting point relates to the structure of the elements. The melting point increases from Group 1 to Group 14 because the elements have giant structures (metallic and then covalent). The melting points decrease from group 14 to 15 because the structure changes to simple molecular, which is only held together by weak intermolecular forces

Metallic bonding is the strong electrostatic attraction between positive metal ions and negative delocalised electrons in a metal lattice

Metals have a fixed lattice structure of positive ions. The outer shell of electrons is delocalised, which can carry current.

Metals have high melting and boiling points due to the large amounts of energy needed to overcome the metallic bonds.

The greater the charge of a metal ion, the more electrons are delocalised. The smaller the size of the metal ions, the closer they are to the delocalised electrons. This results in stronger bonds and a higher melting point

Metals are malleable and ductile. The ions can slide and move past each other as there are no bonds holding specific ions together

X^(n-1) + (g)→ X^n+(g) + e^-

In Period 3:

Aluminium is an exception as the 3s electrons shield the 3p electron

Sulfur is an exception as an electron is being removed from an p orbital containing 2 electrons, so there is electron-pair repulsion

Ionisation energy decreases across a group, as the number of shells increases, so does the atomic radius and shielding, reducing attraction

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A-level Chemistry OCR Notes: Periodicity

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Periodic Table Ionisation Energy Successive ionisation energies apply to the removal of electrons after the first ionisation energy. The nth ionisation energy is:​ Ionisation energy is a measure of the energy required to completely remove an electron from an atom of an element to form an ion.

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A-LEVEL CHEMISTRY CHEATSHEET PACK100 FREE.

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A-LEVEL CHEMISTRY CHEATSHEET PACK100 FREE.

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Your entire course summarised in a handful of pagesEvery spec point coveredAll key definitions, terms, diagrams and processes Beautifully designed by top academic writers & illustratorsAQA, OCR & Edexcel

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- Displays chemical elements arranged by atomic number electron configuration and recurring chemical properties.
- In Mendeleev's time subatomic particles were unknown of.
- Noble gases were emitted from the original table.
- There were only 60 elements in the first periodic table
https://youtu.be/fPnwBITSmgU

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3. First Ionisation Energy

The energy required to remove 1 mol of electrons from 1 mol of gaseous ions

Successive ionisation energies involve removing further electrons

There are smaller trends within a period because full sets of s- and p- orbitals are also stable

P-orbitals are higher in energy than s-orbitals so are further from the nucleus

Further away means lower attraction, so taking an electron from a p-orbital needs less energy

This can be seen going from s- to p-orbitals e.g. Be → B, Mg → Al

Putting an electron into a p-orbital with an electron already in it takes more energy

Successive ionisation energies can be used to work out the electron configuration of an unknown element

A big increase means electrons are being lost from a shell closer to the nucleus

4. Metallic bonding

Metals consist of giant lattices of fixed positive metal ions

These are surrounded by delocalised electrons shared between all the metal ions that can move through the structure

Metallic bonding is the strong attraction between the metal ions and the 'sea' of delocalized electrons

5. Giant covalent lattices

Giant networks of atoms all bonded covalently together e.g. carbon and silicon

Electrons localised in bonds

Three forms of carbon, which forms up to four bonds

1. Each carbon atom forms a single covalent bond to 4 other carbon atoms in a tetrahedral shape

2. Extremely hard because of all the bonds

Silicon as an element has the same structure as diamond

The silicon atoms are where carbon is

One oxygen lies between each silicon atom

6. Properties of giant metal and covalent lattices

Good Conductor of Electricity
Delocalized electrons free to move and carry current even in solid state

Metals aren't soluble, they react with water instead

High melting and boiling boint
Very strong covalent bonds throughout structure need to be broken before melting or boiling occurs

Insoluble, as there are no ions to be solvated

7. Melting points across period 2 and 3

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OCR AS Chemistry Notes: The Periodic Table And Energy - The Periodic Table

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3. First Ionisation Energy The energy required to remove 1 mol of electrons from 1 mol of gaseous ions Successive ionisation energies involve removing further electrons There are smaller trends within a period because full sets of s- and p- orbitals are also stable P-orbitals are higher in energy than s-orbitals so are further from the nucleus Further away means lower attraction, so taking an electron from a p-orbital needs less energy This can be seen going from s- to p-orbitals e.g.

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Learn A Levels, GCSE, KS3 & KS2 2x Faster with Seneca

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Learn A Levels, GCSE, KS3 & KS2 2x Faster with Seneca

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Explains inorganic and physical chemistry, the applications of energy use to everyday life and industrial processes, and current environmental concerns associated with sustainability

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NEW OCR A AS/Yr1 Module 3 - Periodic Table and Energy - YouTube

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OCR A Module 3 - Periodic Table and Energy looks at inorganic and physical chemistry, the applications of energy use to everyday life and industrial processe...

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Reactions of group 2 compounds

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Trends in group 2

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Part 1 & 2

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Periodic Trends In Structure & Melting Point Follow-Up Sheet

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Periodic Trends In Structure & Melting Point Follow-Up Sheet

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Reactions of period 3 elements

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Correlating trends

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Electron configuration and the periodic table

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What do ionisation energies reveal about the atom?

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Periodic Patterns In 1st Ionisation Energies Video 1

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Periodic Patterns In 1st Ionisation Energies Video 1

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Explains what first ionisation energy is and the repeating pattern down groups of the periodic table involving first ionisation energy

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Periodic Patterns in First Ionisation Energies 1

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The process in which an atom loses or gains an electron to become an ion. Ionization energy is a measure of strength of the attraction between the outermost electrons and the nucleus.
First ionization energy- The energy required to remove 1 mole of electrons from 1 mole of gaseous atoms
- Mg(g) ----> Mg⁺(g) + e-
- Period 3 has a general increase in 1st IE with the exceptions of aluminium and sulfur.

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Trends in period 3

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Part 1 & 2

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From Kerboodle

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Covers trends, reactions and properties

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Periodic Patterns In Melting Points Across Period 3 Video

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Periodic Patterns In Melting Points Across Period 3 Video

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Periodic Patterns in Melting Points Across Period 3

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Periodic Patterns In First Ionisation Energies Video 2

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Periodic Patterns In First Ionisation Energies Video 2

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Explains the trend across period 2 of the first ionisation energies and the discrepancies across the period

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Periodic Patterns in First Ionisation Energies 2

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Explains what periodicity is and outlines the difference of observations seen in groups and periods of the periodic table

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Explaining Successive Ionisation Energies Video

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Explaining Successive Ionisation Energies Video

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Explains the reason why ionisation energy increases after each succession and the information you can get from successive ionisation energies

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Explains ionisation energy using oxygen’s 8 ionisation energies

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Covers repeating patterns across a period, successive ionisation energy, ionisation energy and the factors that affect it

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A Level Chemistry - 7 - Electron Structure 2

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Period 3 trends

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Need to know the trends in Period 3 . This is also common to what is seen in other periods

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Flashcards - Periodicity - OCR (A) Chemistry A-Level - PMT

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Flashcards for OCR (A) Chemistry A-Level Topic 3.1.1: Periodicity from Module 3