Summary
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- Module
- Unit 1
- Institution
- PEARSON (PEARSON)
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● what is the atomic structure→The nucleus has positive protons and neutral neutronsand is surrounded by a energy shells with negative electrons.
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● what is the relative atomic mass for protons and neutrons→1
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● what is the relative atomic mass for electrons→almost 0.
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● what is the maximum number of electrons the electron shell one can hold→2
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● what is the maximum number of electrons the electron shell two can hold→8
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● what is the maximum number of electrons the electron shell 3 can hold→18
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● what is the maximum number of electrons the electron shell 4 can hold→32
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● what is the maximum number of electrons the electron shell 5 can hold→50
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● what does Aufbau principle state→Electrons fill orbitals starting at the lowest energy
level and move up.
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● what does orbitals mean→Regions in an atom where electrons are likely to be found.
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● what is the maximum number of electrons an orbital can hold.→2
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● proximity→The state of being near or close to something.
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● Explain electron configuration→This is the distribution of electrons in a molecule or
an atom.
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● why do electrons repel with each other→This is because they have the same charge.
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● what will happen when there is more than one orbital in a sub- shell→They will fill up
singly until all the orbitals in that sub-shell have an electron in them and they will pair
up.
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● what is ionic bonding→This is the electrostatic attraction between two oppositely
charged ions.
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● where are noble gases found in the periodic table→Group 0.
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● Explain why noble gases do not react at all or do not react easily→This is because
they have a full outer shell. And they have a stable electron configuration.
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● why do other elements in the periodic table react→This is because they do not have
a full outer shell, therefore, they react to gain a stable electron configuration.
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, ● when does ionic bonding occur→Ionic bonding occurs when an atom of an element
loses one or more electron and donates it to an atom of a different element.
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● what happens when atoms lose electrons→They become positively charged.
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● what happens when atoms gain electrons→They become negatively charged.
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● Explain what an electrostatic attraction is→This Is the force that experienced by
oppositely charged particles. It holds particles strongly together.
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● what is a Giant ionic lattice→a regular arrangement of of positive and negative ions.
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● what is the strength of electrostatic force of ionic bond dependent on→It is
dependent on the ionic charge and the ionic radii of the ions.
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● what happens when an electron has more positive ions→The more shells it will have.
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● what will happen when an ion has more shells→The radius will be bigger than an ion
with fewer electrons.
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● what happens when ionic charge is high→The electrostatic attraction is stronger.
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● what happens when the ionic radii is bigger→The electrostatic attraction becomes
weaker.
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● Why does the electrostatic attraction become weaker when the ionic radii is
bigger→This is because when the ionic radius is bigger, the ionic charge is spread
over a large surface area.
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● when does an covalent bond occur→between two non-metals.
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● when does a covalent bond form→when an electron is being shared between atoms.
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● where do the electrons come from In a covalent bond→from the top energy level of
an atom.
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● what is a dative covalent bond→A covalent bond where both electrons come from
one of the atoms.
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● what are metals→These are giant structures of atoms held together by metallic
bonds.
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● what is the structure of metal→Regular lattice.
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● what causes metallic bonding→When the electrons from the highest energy level of
an atom has the ability to become delocalised. And they are free to move through the
metal in a 'sea of electrons'. which gives the metal nuclei a positive charge, which is
then attracted to the negative charge of the delocalised electrons.
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