The Periodic Table - History And Use Flashcards

1
Q

Contribution of the greeks?

A

Proposed there were four elements; earth, fire, wind and water.

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2
Q

Contribution of Robert Boyle.

A

Irishman who defined the term element.

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3
Q

Define element.

A

An element is a substance that cannot be split into simpler substances by chemical means. All the atoms in an element have the same atomic number.

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4
Q

Contribution of Humphry Davy

A

Discovered potassium, sodium, calcium, and many other elements by passing electricity through their compounds. (Electrolysis)

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5
Q

Contribution of Dobereiner. Give an example.

A
  • Triads
  • Have similar chemical properties
  • The atomic weight of the middle element is approximately equal to the average of the other two.

Triads: Cl, Br, I ; Li, Na, K

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6
Q

Drawback of Dobereiner’s system.

A

Few triads could be found; deemed a coincidence.

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7
Q

Contribution of John Newlands.

A

If the known elements are arranged in order of their atomic weights, the properties repeat every eight elements.

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8
Q

Drawbacks with Newland’s Octaves.

A

Didn’t take undiscovered elements into account-should have left gaps.
The properties repeat every ninth element in the modern periodic table.
The rules fell apart by the third octave.

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9
Q

Contribution of Mendeleev.

A

Periodic law-elements arranged in order of increasing atomic weight and elements with similar properties placed beneath each other in groups. Left gaps for undiscovered elements and predicted their properties.

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10
Q

What elements did Mendeleev reverse and why?

A

Tellurium was placed before Iodine even though it has a larger atomic weight to ensure it was in the same group as elements with similar properties

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11
Q

Contribution of Moseley.

A

Used x-rays to discover the positive charge of the nucleus. The atomic number. He found that elements in the periodic table are in order of atomic number.

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12
Q

Differences between Mendeleev’s periodic table and the modern periodic table? (5)

A

Mendeleev:

  • Elements arranged in order of increasing atomic weight as opposed to atomic number.
  • Contains gaps for undiscovered elements, modern does not.
  • Only 60 elements; over 100 in modern table.
  • Transition elements not in separate block but are in modern table.
  • No inert gases/noble gases but there are in the modern table.
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13
Q

Contribution and mistakes of Lavoisier.

A

Compiled a list of 33 elements.
E.g. N, C, Cu, Fe
But mistakenly put heat and light in the list.

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14
Q

List the diatomic elements.

A
Hydrogen
Nitrogen
Fluorine
Oxygen
Iodine
Chlorine
Bromine
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15
Q

Describe the reaction of lithium and water in both words and chemical formulae.

A

Lithium + water = lithium hydroxide + Hydrogen

2Li(s) + 2H2O(l) = 2LiOH(aq) + H2(g)

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16
Q

What is the atomic number?

A

Atomic number gives the number of protons in the nucleus.

17
Q

What is the mass number?

A

Mass number gives the total number of protons and neutrons present in the nucleus of an atom.

18
Q

What is an ion? Name for a positive and negative ion.

A

An ion is an atom that has an electrical charge. Positive: Cation. Negative: Anion.

19
Q

How does an atom become an ion?

A

When it gains or loses an electron.

20
Q

What are isotopes?

A

Isotopes are atoms of the same element that have the same atomic number but different mass numbers.

21
Q

Why do isotopes occur?

A

Different atoms can have different number of neutrons in their nuclei.

22
Q

Define Relative atomic mass. Why is it rarely a whole number?

A

This is the average mass of all the isotopes in an element taking abundances into account relative to 1/12th of the carbon 12 isotope. Because it is an average value of all isotopes of an element.

23
Q

How is relative atomic mass measured? Explain it.

A

A mass spectrometer. Isotopes are vaporised, converted into positive ions, accelerated through a magnetic field and are separated according to their mass before being detected at the far end of the tube.

24
Q

Give three uses of mass spectrometry?

A

Identifies presence of isotopes.
Calculates relative atomic mass.
Can detect banned drugs taken by athletes.

25
Q

Define relative atomic mass.

A

The mass of an atom of that element compared with one twelfth of the mass of the carbon-12 isotope.

26
Q

Define relative molecular mass.

A

The mass of a molecule of that substance compared with one twelfth of the mass of the carbon-12 isotope