Topic 1-Atomic Structure and the Periodic table

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  • Created by: McTighe
  • Created on: 06-02-18 18:13
Where is almost all the mass in an atom found?
In the nucleus
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What accounts for the volume of an atom?
The shells of electrons (determines size of atom)
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What nucleons are found in the nucleus?
neutrons and protons
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What charge does the nucleus have?
Positive
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Where are electrons found?
In the surrounding shells
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What is the relative mass of a neutron?
1
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What is the relative mass of a proton?
1
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What is the relative mass of an electron?
1/1840
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What are two other ways to say the proton number?
Atomic number/ Z number
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What is the proton number?
The number of protons inside the nucleus
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What do protons equal?
Electrons
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What is the mass number?
The sum of protons and neutrons in the nucleus of an atom
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How do you work out the number of protons?
Mass number-Proton number
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What is an isotope?
Atoms of the same element which have the same number of protons in the nucleus but different number of neutrons
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What is the relative Isotopic mass?
Mass of one atom relative to 1/12 of the mass of the isotope Carbon-12. It contains one type of Isotope
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What is the relative atomic mass?
The average weighted mass of an atom in an element relative to 1/12 of the mass of an atom in carbon-12. It is not a whole number and is the average for 2 or more isotopes
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What is the relative molecular mass?
Sum of all relative atomic masses of all atoms in its molecular formula (Only applies to molecules)
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What is the relative molecular mass of Sulphuric acid (H2SO$)
(2 X1) + (1 X 32.1) + (4 X 16) = 98.1
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What is the relative formula mass?
Mass of relative atomic masses of all atoms in its formula (Used for giant compounds)
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What does a mass spectrometer do?
Separates atoms and molecules according to their mass and also shows the relative number of different atoms and molecules present
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What are the four steps of mass spectrometry?
-Ionisation -Acceleration -Deflection -Detection
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What state are the atoms and molecules in before they go into the mass spectrometer?
Gaseous
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What is the mass-to-charge ratio?
Depends on mass and charge of an ion
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What mass and charge will cause an ion to deflect more?
Lighter and largely positive
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What does the last line of the mass spectrometer graph show?
The heaviest ion
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What does the tallest line of the mass spectrometer graph show?
The most abundant ion
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Name the diatomic molecule isotopes for chlorine
Chlorine-35+/Chlorine-35+ =70 Chlorine-35+/Chlorine-37+ = 72 Chlorine-37+/Chlorine-37+ =74
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Why does a chlorine ion and molecule form in the ionisation chamber?
An electron is knocked off the ion to form Cl2+. This is not stable so forms a chlorine atom and a Cl+ ion
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What is this a process of?
Fragmentation
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What is Ionisation energy?
The energy required to remove one mole of electrons from one mole of gaseous atoms to produce one mole of positive gaseous ions
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Is it easier to remove an electron if the ionisation energy is higher or lower?
Lower, and therefore makes it more reactive as it can lose an electron more easily
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What is another name for a noble gas?
Inert gas
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Why do noble gases have high ionisation energies?
AS they are most stable due to full outer shells
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Are atoms with half shells stable or unstable?
Quite stable
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Name the three factors that size of ionisation energy
Nuclear charge, Distance from nucleus to the outermost electron, Shielding
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How does Nuclear charge affect the size of ionisation energy?
The more protons in the nucleus, the more positively charged the nucleus is (Greater effective nuclear charge). This causes a stronger attraction for the electrons so more energy is required to overcome the attraction
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How does Distance from nucleus affect the size of ionisation energy?
An electron close the nucleus will be more strongly attracted than an electron further away. Attraction decreases with distance, so less ionisation energy is needed
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How does shielding affect the size of ionisation energy
Electrons in sub-shells closer to nucleus can reduce the full force pulling from the nucleus to outer electrons. More inner electrons means more shielding so a weaker attraction occurs and therefore lower ionisation energy is required
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Does the ionisation energy increase or decrease across a period?
Increase
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Why does the ionisation energy increase across a period?
The elements have more protons in the nucleus, causing a greater effective nuclear charge. They are in the same shell, so same distance from nucleus and same number of inner electrons, causing greater attraction
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Why does ionisation energy decrease down a group?
The outer electron is further away from the nucleus, causing attraction to be weaker. Also has more inner electrons causing attraction to be weaker. There is a greater effective nuclear charge but is outweighed by other factors
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What is the second ionisation energy?
The energy needed to remove a second electron from each ion in one mole of gaseous +1 to give a mole of +2 ions
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Why do successive ionisation energies get larger?
Trying to remove an electron from a positive ion is more difficult as the attraction is stronger, so more energy is required to overcome the attraction
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What is the Emission Spectrum?
A spectrum of the electromagnetic radiation emitted by a source
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What is the Absorption Spectrum?
A spectrum of electromagnetic radiation transmitted through a substance showing dark lines due to absorption of specific wavelengths
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What is the ground state?
The lowest energy, most stable electron arrangement of an atom
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How can hydrogen emission spectrum be seen?
When light is passed through a prism or diffraction grating. It splits into various colours which is part of the spectrum
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Why are their different lines of the emission spectrum?
Energy is absorbed by the atoms to promote electrons to a higher energy level.These will eventually fall back to ground state and emit energy.
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What is the flame colour of Potassium?
Lilac
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What is the flame colour of Calcium?
Brick red
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What is the flame colour of Strontium?
Red
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What is the flame colour of copper?
Green
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What is the flame colour of sodium?
Yellow/Orange
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What is the flame colour of Barium?
Green
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What is the flame colour of Lithium?
Red
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Name three of hydrogens series
Lyman (UV Light), Balmer (partly visible), Paschen (Infrared)
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What is the infinity level?
Represents the highest possible energy an electron can havee as part of a hydrogen atom. If an electron exceeds this, it is no longer apart of the atom as ionisation occurs (positively charged ion)
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What is the ionisation energy per electron?
Measure of the distance between 1st level and infinity level
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How many electrons can each orbital hold?
2 electrons
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How many orbitals are in the s subshell?
1 orbital
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How many orbitals are in the p subshell?
3 orbitals
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How many orbitals are in the d subshell?
5 orbitals
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How many orbitals are in the f subshell?
7 orbitals
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Which subshells are found in 1st shell?
s
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Which subshells are found in 2nd shell?
s,p
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Which subshells are found in 3rd shell?
s,p,d
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What are orbitals?
Space the electron is most likely to exist (Heinsberg's uncertainity)
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Does 3d have less or more energy than 4s?
more (3s 3p 4s 3d)
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What is the S-orbital?
Spherically symmetric around nucleus (one orbital)
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What is the P-orbital?
2 identical spheres tied together at the nucleus (Petal). They point in particular direction. The electrons move in opposite directions
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What is the D and F-orbitals?
at the third level, there are 5 sets of d orbitals, at the forth level, there are 7 sets of f orbitals
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What are the three rules of electron configurations?
1.Electrons go into orbital with lowest available energy level first 2.Each orbital only contains two electrons on opposite spins 3.Where there are two more orbitals at the same energy, they fill singulary first
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What does periodicity mean?
Repeating patterns across different periods
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What are the vertical groups on a periodic table?
All elements in the group have similar electrons due to the fact they have the same number of outer electrons
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What are the horizontal periods on a periodic table?
All have same number of shells. Properties of an element in the same period change gradually moving from one side to another
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Card 2

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The shells of electrons (determines size of atom)

Card 3

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What nucleons are found in the nucleus?

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Card 4

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What charge does the nucleus have?

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Card 5

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Where are electrons found?

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