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
2) Acceleration
3) Deflection
4) Detection

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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:
- further away from the nucleus

- 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?
answer

PV = nRT

P = Pressure in Pa
V = Volume in m3

T = temperature in K

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