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Chemistry > Peridoic Table > Flashcards

Peridoic Table Flashcards

1
Q

First ionisation energy

A

The minimum energy required to remove the most loosely bound electron from a NEUTRAL GASEOUS atom in its ground state

Decreases down a group
Increases across a period

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2
Q

Electron configuration

A

Shows the arrangement of electrons in the atom of an element

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3
Q

Aufbau principle

A

When building up the electron configuration of an atom in its ground state, the electrons occupy the lowest energy level available

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4
Q

Hund’s Rule of Maximum Multiplicity (bus seat rule)

A

When 2+ orbitals of equal energy are available, the electrons occupy them singly before filling in pairs

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5
Q

Pauli Exclusion Principle

A

No more than 2 electrons can occupy an orbital and they must have an opposite spin

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6
Q

An element

A

A substance that can’t be split into simpler substances by chemical means

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7
Q

Newland’s Octaves

A

Arrangements of electrons when the 1st and 8th elements have similar properties

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8
Q

Triad

A

A group of 3 elements of similar properties, where the Relative Atomic mass of the middle element is the average of the other two elements

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9
Q

Mendeleev’s Periodic Law

A

When elements are arranged in order of increasing Relative Atomic mass (atomic weight) the properties of the elements recur periodically

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10
Q

Recur periodically

A

Repeat at regular intervals

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11
Q

Atomic number of an atom

A

The amount of protons (H+) in the nucleus of an atom

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12
Q

Modern periodic table

A

An arrangement of atoms in order of increasing atomic number

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13
Q

Modern Periodic Law

A

When elements are arranged in order of increasing atomic number, the properties of the elements recur periodically

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14
Q

Mass number

A

The sum of protons+neutrons in the nucleus

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15
Q

Isotopes

A

Atoms of the same element with different mass numbers due to a different number of neutrons in the nucleus

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16
Q

Relative Atomic mass

A

The average of the mass numbers of all the isotopes as they occur naturally, taking their abundance’s into account and expressed on a scale where the atoms of carbon-12 has a mass of 12 units

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17
Q

Principle of Mass Spectrometry

A

Charged particles moving in a magnetic field are deflected to different extents according to their mass numbers

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18
Q

Electronegativity

A

The relative attraction an atom in a molecule has for the shared pair of electrons in a covalent bond

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19
Q

Atomic radius

A

Half the distance between the nuclei of 2 atoms of the same element that are joined by a single covalent bond

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20
Q

Value of atomic radius….increase/decrease

A

Increases down the group (screening effect)

Decreases across a period (no increase in screening effect)

21
Q

Second ionisation

A

The energy required to remove an electron from an ion with one positive(+) charge in the gaseous state

22
Q

Value of electronegativity….increase/decrease

A

Increases across the periods (decreasing atomic radius/ increasing effect of nuclear charge)

Decreases down the groups (increasing atomic radius)

23
Q

Value of first ionisation energy…increase/decrease

A

Increases across a period (decreasing atomic radius)

Decreases down a group (increasing atomic radius/screening effect)

24
Q

4 original elements (Greek philosophers)

A

Water, fire, earth, air

25
Q

Contribution of Robert Boyle

A

Defined an element as: a substance that can’t be split into simpler substances by chemical means

26
Q

Why is water not an element.

A

Water is a compound and not an element as it can be split into simpler substances, Hydrogen and Oxygen

27
Q

How did Davy discover potassium (K)?

A

Passing electricity through a compound of K

Also discovered: Na, Mg

28
Q

Dobereiner’s contribution

A

Discovering triads

E.g. li, Na, K

29
Q

Atomic weight=

A

Relative Atomic mass

30
Q

Important chemists into devising the periodic table

A

Dobereiner (triads)
Newland (octaves)
Mendeleev (Mendeleevs Periodic Law)
Moseley (Atomic number)

31
Q

Problem with Newland’s Octaves?

A

Noble gases weren’t in it because they hadn’t been discovered
Didn’t leave gaps

32
Q

Summarise Mendeleev’s work/Periodic Table

A
  1. Left gaps
  2. Elements with similar properties in same vertical column (properties repeated periodically)
  3. Predicted properties of undiscovered elements (predicted properties of Germanium & Gallium before discovery)
  4. Reversed the order of some elements
33
Q

Why is Tellirium before Iodine?

A

Mendeleev arranged his table in order of increasing atomic weight, but Te has a higher weight than I and yet is before it, as he realised the properties were more important than their weights, by reversing them the elements were in groups of similar properties

34
Q

Moseley’s contribution to the Periodic Table?

A
  1. Discovered the atomic number of an atom
  2. Arranged the table in order of increasing atomic number (elements now fall naturally into groups, no reversing)
  3. Confirmed Mendeleev was right placing Te before I
35
Q

Differences between Mendeleev’s Periodic Table and the Modern Periodic Table?

A 
1. Mendeleev: increasing atomic weight 
Modern: increasing atomic number 
2. Mendeleev: gaps 
Modern: no gaps 
3. Mendeleev: some elements not discovered (noble gases)
Modern: more elements
36
Q

Important uses of the Periodic Table?

A

Finding atomic no. and mass no.
Finding relative Atomic mass
Electron configuration

37
Q

Number of neutrons?

A

Mass no.-Atomic no.

38
Q

Who built the mass spectrometer?

A

William Aston- to measure the masses of atoms

Aston also discovered isotopes

39
Q

Isotopes of carbon?

A

Carbon-12, carbon-13, carbon-14

40
Q

3 Isotopes of hydrogen?

A

Hydrogen-1, hydrogen-2, hydrogen-3

41
Q

5 processes in mass spectrometry

A 
Vaportpisation 
Ionisation 
Acceleration 
Separation in a magnetic field 
Detection

VIASD (Volumes In Acids Stay Donating)

42
Q

What is a mass spectrometer used for?

A

To identify isotopes, their abundance’s and the relative atomic mass of an element
To identify unknown compounds

43
Q

Use of mass spectrometer for identifying unknown compounds?

A

Chromatography- to detect banned drugs taken by athletes

Drug tests- drugs leave traces in the addict’s hair

44
Q

Bohr’s electronic configuration of Potassium?/ showing the no. Of electrons in each main energy level

A

2,8, 8, 1

45
Q

Electronic configuration of Cr and Cu (odd ones out)

A

Cr: 1s2, 2s2, 2p6, 3s2, 3p6, 4s1, 3d5

Cu: 1s2,2s2, 2p6, 3s2, 3p6, 4s1, 3d10

(This provides extra stability- 4s sublevel being half filled)

46
Q

Why is the 4s sublevel filled before the 3d sublevel?

A

4s sublevel has less energy

47
Q

When are sublevels extra stable?

A

When they completely filled or half filled

48
Q

Ion

A

A charged atom
(Has lost or gained electrons)

Atom loses electrons—> positively charged
Atom gains electrons—> negatively charged

49
Q

Reactivity of alkali metals…increases/decreases?

A

Very reactive (low first ionisation energy+a single electron in the outer energy level to be lost)

Increases down the group (increasing atomic radius)

Chemistry (12 decks)

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