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