electronic structure & bonding and structure summary
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Course
AS Unit F321 - Atoms, Bonds and Groups
Institution
OCR
detailed notes on content in module 2 including:
electronic astructure and configuration, bonding and structure, types of intermolecular forces and shapes of covalent molecules
diagrams to aid learning
Answer: region around the nucleus that can hold up to 2 electrons, with opposite spins
2.
electro notation order
Answer: 1. energy level
2. sub shell
3. orbital
3.
shapes of orbital
Answer: spherical and dumbbell-shaped
4.
which type of orbital is spherical ?
Answer: s orbital
5.
types of subshells
Answer: s, p, d, f
ionic and covalent + coordinate bonds
Flashcards35 Flashcards
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Flashcards35 Flashcards
R66,940 sales
Some examples from this set of practice questions
1.
ionic bond is between which types of atoms?
Answer: metal and non metal
2.
exception of an ionic bond
Answer: NH4Cl
3.
ionic bond occurs in which groups of the periodic table?
Answer: 1,2 , d block except Al
4.
definition of an ionic bond
Answer: strong electrostatic attraction between positive and negative ions
5.
3 propertes of ionic bonds
Answer: static, fixed electrons and static charge
shapes of covalent bonds and electronegativity
Flashcards55 Flashcards
R66,940 sales
Flashcards55 Flashcards
R66,940 sales
Some examples from this set of practice questions
1.
why do covalent molecules have different shapes ?
Answer: have different number of bond and lone pairs of electrons
2.
what is a lone pair of electrons ?
Answer: not involved in covalent bonding
3.
what is a bond pair of electrons ?
Answer: involved in covalent bonding
4.
which type of electron pairs repel more strongly ?
Answer: lone pairs
5.
why do lone pairs repel more strongly than bond pairs ?
Answer: they are closer to the central atom, occupying more space than a bonded pair
bonding and structure, intermolecular forces
Flashcards71 Flashcards
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Flashcards71 Flashcards
R78,140 sales
Some examples from this set of practice questions
1.
3 types of intermolecular forces
Answer: london forces, permanent dipole-dipole interactions and hydrogen bonds
2.
what is meant by intermolecular forces ?
Answer: forces acting between molecules
3.
are ionic, covalent bonds types of intermolecular forces?
Answer: No because they act within molecules
4.
london forces can also be called ...
Answer: induced dipole-dipole interactions
5.
london forces occur when ..
Answer: random electron movement causes a temporary dipole, which induces a further temporary dipole in neighbouring molecules.
Content preview
ELECTRONIC STRUCTURE
Electrons have fixed energies and move around the nucleus in shells / energy levels
(principal quantum number)
Shells further from the nucleus have a higher energy and a larger principal quantum
number than shells closer to the nucleus
Shells are divided into sub shells
Different electron shells have different numbers of sub shells with a different energy
Sub shells have different number of orbitals that can hold up to 2 electrons
Sub shells : s-, p-, d-, f- .
S: 1 orbital =2 e-
P: 3 =6e-
D: 5 = 10e-
F: 7 =14e-
An orbital is an area around the nucleus in which an electron moves in
Orbitals within the same sub-shell have the same energy
2 electrons in a orbital spin in opposite directions = spin pairing
S orbital is spherical
P orbital is dumbbell shaped ( 3p orbitals at right angles to one another)
Shells and total number of electrons
1st: 2
2nd: 8
3rd: 18
4th: 32 (sum of all other electrons in other orbitals)
, ELECTRONIC CONFIGURATION (number of electrons and how they’re arranged)
1 box= orbital
1 arrow = electron
Up & down arrows = electrons spinning in opposite directions
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