CH1 - Basic ideas about atoms
- Created by: zopetre_
- Created on: 12-04-17 18:48
What is the mass and charge of a proton, neutron a
Proton has the mass of 1 and charge of +1
Neutron has the mass of 1 and charge of 0
Electron has a negligible mass (1/1840) and a charge of -1
What happens if an atom loses one or more electron
It forms a positive ion/cation.
What happens if an atom gains one or more electron
It forms a negative ion/anion.
What is radioactive decay?
Where unstable isotopes split up to form smaller atoms. This happens as the nucleus divides and sometimes protons, neutrons and electrons fly out. The element is said to be radioactive.
Describe alpha particles
Alpha particles consist of two protons and two neutrons, therefore helium nuclei
They are the least penetrating of the three types of radiation and are stopped by a thin sheet of paper or even a few cm of air
They are positively charged
Describe beta particles
High-energy electrons that are more penetrating than alpha radiation
They can travel through up to 1m of air, but they're stopped by a 5mm thick sheet of aluminium
They are negatively charged
Describe gamma rays
High-energy electromagnetic waves which are the most penetrating type of radiation
They can pass through several cm of lead or more than a metre of concrete
They have no charge
Describe the effect of an electric field on radiat
Gamma rays are undeflected
Alpha particles are deflected towards the negative charge, proving positive
Beta particles are deflected towards the positive charge, proving negative
Describe the effect of a magnetic field on radiati
When a charged particle cuts through a magnetic field it experiences a force referred to as the motor effect.
Alpha particles are deflected towards the negative charge, proving positive
Beta particles are deflected towards the positive charge, proving negative
Gamma rays are unaffected by the magnetic field, showing they have no charge
What happens when an element emits an a particle?
Its mass number decreases by 4 and its atomic number decreases by 2
The product is two places to the left in the periodic table
What happens when an element emits a b particle?
Its mass number is unchanged and its atomic number increases by 1
The product is one place to the right in the periodic table
What happens when an element emits an electron neu
It's a process of inverse beta decay, atomic number decreases by 1
Product is one place to the left in the periodic table
e.g X + e- > X
What happens to an element during positron emissio
Atomic number decreases by 1
Product is one place to the left in the periodic table
e.g X > X + B+
What are the consequences of radiation on living c
Damages the DNA, leading to mutations and possibly the formation of cancerous cells.
Gamma radiation is the most dangerous outside of the body, but inside the body alpha is more dangerous.
How is radioactivity beneficial in medicine?
Cobalt-60 is used in radiotherapy for cancer treatment. High energy gamma rays kill cancer cells, preventing malignant tumours from forming.
Technetium-99m is used as a medical radioisotope. It's used as a tracer to label a molecule which is taken up by the tissue to be studied.
How is radioactivity beneficial in radio-dating?
Carbon-14 is used to calculate the age of plant and animal remains
Potassium-40 is used to estimate the geological age of rocks
How is radioactivity beneficial in analysis?
Dilution analysis in the use of isotopically labelled substances to find the mass of a substance in a mixture
Measuring the thickness of metal strips or foils
Describe the different types of subshells
S subshell which can hold 2 electrons
P subshell which can hold 6 electrons
D subshell which can hold 10 electrons
F subshell which can hold 14 electrons
What are the rules for filling orbitals with elect
1) Electrons fill atomic orbitals in order of increasing energy (Aufbau principle)
2) A max of 2 electrons can occupy any orbitial each with opposite spins (Pauli exclusion principle)
3) The orbitals will first fill with 1 electron each with parallel spins, before a second is added with a paired spin (Hund's rule)
What are the equations for the first few ionisatio
First: X(g) > X+(g) + e-
Second: X+(g) > X2+(g) + e-
Third: X2+(g) > X3+(g) + e-
etc
What are the factors affecting the ionisation ener
Size of positive nuclear charge - greater charge, greater attractive force on outer electron, greater the ionisation energy
Distance of outer electron from nucleus - force of attraction between the nucleus and outer electron decreases as the distance between them increases, the further an electron from the nucleus, the lower the ionisation energy
Shielding effect - electrons repel each other as they're negatively charged, electrons in filled inner shells repel electrons in outer shells, reducing effect of positive nuclear charge, more filled inner shells, smaller attractive force on outer electron, lower the ionisation energy
Equation relating frequency and wavelength of ligh
c = fλ (c = speed of light)
Equation relating the frequency of electromagnetic
E = hf (h is Planck's constant)
Describe the relationship between frequency and en
f ∝ E
If frequency increases, energy increases.
Describe the relationship between frequency and wa
f = 1/λ
If frequency inceeases, wavelength decreases
Describe the absorption spectra
When white light is passed through the vapour of an element, certain wavelengths are absorbed by the atoms and removed from the light.
When you look through a spectrometer, black lines in the spectrum show where light of some wavelengths has been absorbed.
Wavelengths correspond to the energy taken in by the atoms to promote them to higher energy levels.
Describe the emission spectra
When atoms are given energy the electrons become excited, and the energy promotes them to higher energy levels
When the energy is removed, the electrons leave the excited state and fall from the higher energy level, releasing the energy as a photon with a specific frequency
This is shown as coloured lines on a black back ground
Describe the hydrogen spectrum
One electron, simplest emission spectrum.
Atom excited by energy, electron jumps to a higher energy level. When it falls back down it emits energy as a photon, and it can be seen as a line in the spectrum.
Each line in the Lyman series is due to an electron returning to n=1, while the Balmer series is due to electrons returning to n=2.
Describe the ionisation of the hydrogen atom
Spectral lines become closer together as frequency increases until they converge to a limit
Convergence limit corresponds to the point at which the energy of an electron is no longer quantised and the nucleus has lost control over the electron, the atom is ionised
Lyman series n = 1, convergence limit represents the ionisation of the hydrogen atom.
How do you calculate ionisation energy?
ΔE = hf
Δ x Avogadro's constant = 1st I.E for a mole of atoms
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