Term
What is the Relative Atomic Mass (Ar)?
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Definition
The average mass of an atom of an element compared to 1/12 of the mass of an atom of carbon-12 |
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Term
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Definition
The mass in grams of one mole of particles (The top number on Periodic Table)
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Term
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Definition
| The measure of the number of particles |
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Term
What is the Empirical Formula?
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Definition
The simplest ratio of atoms of each element in a compound
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Term
| What is the Molecular Formula? |
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Definition
| The actual number of atoms of each element in a molecule |
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Term
| What is the Relative Mass and Relative charge of a Proton? |
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Definition
Relative Mass: 1 Relative Charge: +1 |
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Term
| What is the Relative Mass and Relative Charge of a Neutron? |
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Definition
Relative Mass: 1 Relative Charge: 0 |
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Term
| What is the Relative Mass and Relative Charge of an Electron? |
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Definition
Relative Mass: 1/1800 Relative Charge: -1 |
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Term
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Definition
| The number of protons and neutrons in the nucleus of an element (A) |
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Term
| What is the Atomic Number? |
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Definition
| The number of protons in the nucleus (Z) |
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Term
| What is an isotope of an element? (Physical and Chemical properties?) |
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Definition
Has the same number of protons BUT a different number of neutrons Physical properties of isotopes differ Chemical properties of isotopes are the same |
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Term
| Name the 4 stages of Mass Spectrometry |
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Definition
1) Ionisation
2) Acceleration
3) Deflection
4) Detection |
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Term
Describe the process of ionisation
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Definition
| Electrons from the electron gun is fired into the sample and knocks off the outermost electon forming a unipositive ion |
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Term
What is the general equation for ionisation?
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Definition
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Term
How does acceleration occur in mass spectrometry?
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Definition
| A negative electric field accelerates the beam of postive ions and slits narrow it |
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Term
Describe how deflection occurs
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Definition
| The fast moving beam of positive ions is deflectd by variable magnetic field |
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Term
| For a given magnetic field: the greater the mass... |
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Definition
the less the ions are deflected
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Term
For a given magnetic field: the greater the postive charge...
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Definition
| the more they are deflected |
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Term
| Describe the process of detection |
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Definition
| When a positive ion reaches the detecter, a tiny current is produced. The signal is fed to a recorder. |
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Term
Why do the chemical properties of isotopes stay the same?
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Definition
Because there are the same number of electrons and electron configuration
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Term
Recite the electronic configuration pattern
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Definition
1s2 2s2 2p6 3s2 3p6 3d10 4s2 4p6 4d10 4f14
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Term
| As you go down Group II from beryllium to barium... |
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Definition
| there is a succesive decrease in first ionisation energy |
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Term
There is a decrease in ionisation energy as you go down Group II because....
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Definition
The outer electron is:
- further away from the nucleus - more shielded from nuclues by inner electrons SO electron is more easily removed |
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Term
As you go across Period 3...
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Definition
| there is a general increase in ionisation energy |
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Term
| There is a general increase in ionisation energy as you go across Period 3 because... |
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Definition
the nuclear charge in each element increases and so the electrons are attracted more strongly and it takes more energy to remove
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Term
| There is a fall in ionisation energy from magnesium to aluminium because... |
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Definition
| the outer electron in aluminium is in a p sublevel (higher energy level than s sublevel of magnesium) |
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Term
The fall in ionisation energy from Phosphorus to Sulphur is because...
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Definition
| the electrons are paired in the 3p sub level of Sulphur. This means they repel each other and are less attracted to the nucleus. |
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Term
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Definition
| The bond formed between two non-metals (they share electrons) |
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Term
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Definition
| The bond formed between a positive metal and a negative non-metal (transferring of electrons) |
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Term
| What is Avogadro's Constant (L)? |
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Definition
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Term
How many particles does 1 mole of a substance contain?
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Definition
| 6.023 x 1023 (Avogadro's Constant) |
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Term
What is the equation for the Number of moles?< |
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Definition
Mass (g)
Molar Mass (gmol-1) |
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Term
What is the Ideal Gas Equation?
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Definition
PV = nRT P = Pressure in Pa
V = Volume in m3 T = temperature in K |
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