Summary

Summary Ions - Unit 1 - Principles and Applications of Science I

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Course
Unit 1 - Principles and Applications of Science I

Institution
PEARSON (PEARSON)

These notes contain summary notes on the topic Ions in chemistry. They helped me achieve distinction overall and are easy to understand. These notes also contain information on the topics - Empirical Formula, Ionic Compounds, Dot and Cross Diagrams, Ionic Bonding, and Atoms.

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Uploaded on May 15, 2023
Number of pages 6
Written in 2022/2023
Type Summary

ions
empirical formula
ionic compounds
dot and cross diagrams
ionic bonding
atom

Study Level
BTEC
Examinator
PEARSON (PEARSON)
Subject
Applied Science 2016 NQF
Unit
Unit 1 - Principles and Applications of Science I

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Bonds (Ionic)

Ions:

 Is an atom or group of atoms with a positive or negative charge.
 Atoms sometimes lose or gain electrons (e.g. when a metal reacts with anon-metal). When they
do this they become a charge atom or an ion.
 If an atom loses 1 or more electrons, it gains a positive charge because it has less electrons than
protons.
E.g. if sodium atom loses 1 electron, it forms a Na+ ion.
It has 11 protons, 12 neutrons and 10 electrons.
 If an atom gains 1 or more electrons, it gains a negative charge beause it has more electrons
than protons.
2-
E.g. if an oxygen atom gains 2 electrons, it forms a 0 ion.
It has 8 protons, 8 neutrons and 10 electrons.

Ionic Bonding:

 Ionic bonds form between metal and non-metals.
 Ionic bonding consists of electrons moving from 1 atom to
another. This then produces cations (+) and anions(-)
An ion is an atom or group of atoms with a positive or negative charge.
 Metals lose electrons to become positively charged ions
 Non-metals gain electrons to become negatively charged ions.

POSITIVE IONS NEGATIVE IONS
Hydrogen H+ Fluorine F-
Lithium Li+ Chloride Cl-
Sodium Na+ Bromide Br-
Potassium K+ Iodide I-
Magnesium 2+ Oxide -
Mg O2
Calcium 2+ Hydroxide OH-
Ca
Aluminum 3+ Nitrate
Al NO3 -
Silver Ag+ Sulphate 2-
SO4
Copper 2+ Phosphate 3-
Cu PO4
Ammonium Carbonate 2-
NH4 + CO3
Iron 2+ 3+
Fe & Fe
*They have all lost electrons *These have all gained electrons
*They’re all metals apart from H+ and NH 4 + *They’re all non-metals
*The elements in Group 1 react with the elements in Group 7.
*Groups 1 elements can each lose 1 electron.
This electron can be given to an atom from Group 7, they both achieve the stable electronic
structure of a noble gas.

1

, Bonds (Ionic)

Dot and Cross Diagrams:

 The electrostatic attraction between the oppositely charged Na+ ions and Cl- ions is
called ionic bonding. The electron transfer during the formation of an ionic compound
can be showed through dot and cross diagram:

 The charge on the ions produced by metals in group 1 and 2 and by non-metas in group 6 and 7
relates to the group number of the element in the periodic table.
For example; Group 1 form 1+ ions, Group 3 form 3+ ions, Group 6 form 2- ions and Group 7
form 1- ions.

Examples;

 Magnesium Oxide:
Sometimes the atoms reacting need to gain or lose 2 electrons to gain a stable noble gas
structure. Each magnesium loses 2 electrons and each oxygen gains 2 electrons.
2+
Magnesium ions have the formula Mg , while oxide ions have the formula O2- .
This means that 1 magnesium atom reacts with 1 oxygen atom, giving the formula MgO

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