Structure and Bonding

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  • Created by: LBCW0502
  • Created on: 15-10-17 09:00
A good understanding of chemistry is needed for what? (5)
Design/synthesis of new drugs, understand effect of drugs, understand drug interactions in living organisms, predict drug properties and how drugs are controlled for purity
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What are atoms?
The simplest building blocks which can form elements
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What is an element?
A substance made up of only one type of atom and cannot be separated into simpler substances via chemical reactions
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What is a compound/molecule?
A substance made up of two or more different types of atoms chemically bonded in fixed proportions
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What is the periodic table?
A tabular arrangement of elements in vertical columns (groups) and rows (periods) based on similar chemical properties (ratios with oxygen)
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Which atomic theory did Democritus and Dalton develop?
Round sphere with no protons, electrons and neutrons. All matter was composed of atoms (cannot be divided)
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Which atomic theory did Thomsom develop?
Plum Pudding Model - mix of positive and negative charge in nucleus
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Which atomic theory did Rutherford develop?
Atom made up of empty space with large positive nucleus (Geiger-Marsden experiment)
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Which atomic theory did Bohr develop?
Electrons are in discrete energy levels
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What is the Modern Quantum Cloud Model?
Mathematical equations used to find location of electrons in atoms (in the orbitals)
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What is the size of an atom?
10^-10 m
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What is the size of a nucleus?
10^-14 m
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What does the central nucleus contain?
Protons and neutrons
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What are the masses of a proton and a neutron?
They each have a mass of 1 amu
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What are the charges of a proton and a neutron?
A proton has a +1 charge and a neutron has 0 charge
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What is the overall charge on a nucleus?
Positive
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The outer arrangement (orbitals) contains which type of sub-atomic particle?
Electrons
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What is the mass of an electron?
1/1837 amu
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What is the charge of an electron?
-1
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What is the overall charge on an atom?
Neutral (0) - number of protons equals the number of electrons
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Which sub-atomic particles contribute to the mass of an atom?
Protons and neutrons
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Which sub-atomic particles contribute to the charge of an atom?
Protons and electrons
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What does Z mean?
Atomic number (number of protons)
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What does N mean?
Number of neutrons
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What does A mean?
Mass number (A = Z + N)
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What are isotopes?
Atoms of a particular element that have the same number of protons (and electrons) but different numbers of neutrons (they have different mass numbers)
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What are the isotopes of hydrogen?
Protium, deuterium and tritium
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How can elements be converted to other elements?
Through nuclear reactions e.g. hydrogen converted to helium
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What are chemical bonds?
Electrostatic forces of attraction which hold atoms of elements together in a compound
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What are ionic compounds?
Electrons lost (metals/cations) or gained (non-metals/anions) through a transfer. Strong electrostatic forces of attraction between oppositely charged ions
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What are covalent compounds?
Electrons are shared between non-metals
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What are cations?
Positively charged ions
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What are anions?
Negatively charged ions
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What are the ways of presenting a formula? (3)
Molecular formulae, structural formulae or molecular model (ball and stick or space filling type)
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What is dimerisation?
Monomers are linked together through hydrogen bonds, coordinate bonds or covalent bonds
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What are the key points in the Bohr Model of the atom?
Electrons lose energy, arranged in discrete energy levels, principle energy levels/electrons shells, shells are filled in order of increasing energy
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Why is the Bohr Model of the Atom wrong?
Electrons in atoms don't occupy simple circular orbits
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How do electrons behave similarly to? (2)
Particles and waves
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The square of a wave function is proportional to what?
The probability to find an electron in a given space
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Each wave function is described by what?
Four quantum numbers - each different orbital has its own individual quantum numbers
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What is n?
Principle quantum number - values of n divide orbitals into groups with similar energies (shells)
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What is l?
Orbital angular momentum quantum number - tells us the shape of the orbital and can have any value, usually given letters: s, p, d, f
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What is m?
Magnetic quantum number - determines orientation of angular movement - where orbitals are in space (+/-)
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What is s?
Spin angular momentum quantum number - (+/- 0.5) two electrons occupy the same orbital but must have opposite orientation/spin
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Which orbital has a very high probability of finding an electron?
1s orbital
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What is the Heisenberg Uncertainty Principle?
Position/momentum (MxV) cannot be both known to arbitrary precision. More precise one is known, the less precise the other is known (Quantum Mechanics phenomenon)
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Describe an s orbital
Sphere shaped, symmetrical, boundary surface, high probability of finding an electron
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Describe a p orbital
There are three p orbitals, dumb-bell shaped, 2 lobes, nodal plane (region with no electron density), three types of orientation
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Describe a d orbital
Don't usually focus on
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Describe an f orbital
More complex
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What is the Aufbau principle?
Electrons enter orbitals of progressively higher energy
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What is the Pauli exclusion principle?
An orbital holds a maximum of two electrons
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What is Hund's rule?
Equivalent orbitals are half-filled before a second electron enters to be completely filled
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What are the key aspects when drawing electronic configuration? (3)
Using rules, arrows (electrons), boxes (orbitals)
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What are valence electrons?
Electrons in the outermost shell, interact in chemical reactions, reactivity depends on readiness to interact (ready-reaction, reluctant-no reaction)
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What are core electrons?
Completely filled orbitals, don't take part in a chemical reaction
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What is a Lewis structure?
Shows symbol for element, shows outermost electrons/valence electrons as dots or crosses. Covalent bond (a dash line), lines are used for bonds
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How do you draw a Lewis structure?
Count/add the number of valence electrons from each atom in the molecule/ion. Determine arrangement, subtract electrons used in bonds (2) from total, assign remaining electrons using Lewis rules, correctness
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What is the octet rule?
Period 2 or 3 atoms will have a complete octet, hydrogen atoms will have a 'pair'
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What is in a single bond?
1 shared pair of electrons
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What is in a double bond?
2 shared pair of electrons
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What is in a triple bond?
3 shared pair of electrons
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Which atom is always singly bonded?
Hydrogen atom
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What are lone pairs?
Electrons not involved in forming bonds (arranged in pairs)
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Which elements form incomplete octet structures?
Group three elements (B, Al). They form three bonds. Due to small energy group (promotion of electron - extra energy released in bond making)
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Due to promotion, carbon forms how many bonds?
4
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Which groups promote electrons to form more bonds?
Groups, 2, 3 and 4
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Which atoms form expanded octet structures?
Phosphorous (5 bonds), and sulfur (6 bonds). 3d orbitals available (all due to promotion of electrons)
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Card 2

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What are atoms?

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The simplest building blocks which can form elements

Card 3

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What is an element?

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Card 4

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What is a compound/molecule?

Back

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Card 5

Front

What is the periodic table?

Back

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