Peridoic Table

Question 1

First ionisation energy

Answer 1

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

Question 2

Electron configuration

Answer 2

Shows the arrangement of electrons in the atom of an element

Question 3

Aufbau principle

Answer 3

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

Question 4

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

Answer 4

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

Question 5

Pauli Exclusion Principle

Answer 5

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

Question 6

An element

Answer 6

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

Question 7

Newland’s Octaves

Answer 7

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

Question 8

Triad

Answer 8

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

Question 9

Mendeleev’s Periodic Law

Answer 9

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

Question 10

Recur periodically

Answer 10

Repeat at regular intervals

Question 11

Atomic number of an atom

Answer 11

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

Question 12

Modern periodic table

Answer 12

An arrangement of atoms in order of increasing atomic number

Question 13

Modern Periodic Law

Answer 13

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

Question 14

Mass number

Answer 14

The sum of protons+neutrons in the nucleus

Question 15

Isotopes

Answer 15

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

Question 16

Relative Atomic mass

Answer 16

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

Question 17

Principle of Mass Spectrometry

Answer 17

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

Question 18

Electronegativity

Answer 18

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

Question 19

Atomic radius

Answer 19

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

Question 20

Value of atomic radius….increase/decrease

Answer 20

Increases down the group (screening effect)

Decreases across a period (no increase in screening effect)

Question 21

Second ionisation

Answer 21

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

Question 22

Value of electronegativity….increase/decrease

Answer 22

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

Decreases down the groups (increasing atomic radius)

Question 23

Value of first ionisation energy…increase/decrease

Answer 23

Increases across a period (decreasing atomic radius)

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

Question 24

4 original elements (Greek philosophers)

Answer 24

Water, fire, earth, air

Question 25

Contribution of Robert Boyle

Answer 25

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

Question 26

Why is water not an element.

Answer 26

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

Question 27

How did Davy discover potassium (K)?

Answer 27

Passing electricity through a compound of K Also discovered: Na, Mg

Question 28

Dobereiner’s contribution

Answer 28

Discovering triads | E.g. li, Na, K

Question 29

Atomic weight=

Answer 29

Relative Atomic mass

Question 30

Important chemists into devising the periodic table

Answer 30

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

Question 31

Problem with Newland’s Octaves?

Answer 31

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

Question 32

Summarise Mendeleev’s work/Periodic Table

Answer 32

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

Question 33

Why is Tellirium before Iodine?

Answer 33

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

Question 34

Moseley’s contribution to the Periodic Table?

Answer 34

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

Question 35

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

Answer 35

``` 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 ```

Question 36

Important uses of the Periodic Table?

Answer 36

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

Question 37

Number of neutrons?

Answer 37

Mass no.-Atomic no.

Question 38

Who built the mass spectrometer?

Answer 38

William Aston- to measure the masses of atoms Aston also discovered isotopes

Question 39

Isotopes of carbon?

Answer 39

Carbon-12, carbon-13, carbon-14

Question 40

3 Isotopes of hydrogen?

Answer 40

Hydrogen-1, hydrogen-2, hydrogen-3

Question 41

5 processes in mass spectrometry

Answer 41

``` Vaportpisation Ionisation Acceleration Separation in a magnetic field Detection ``` VIASD (Volumes In Acids Stay Donating)

Question 42

What is a mass spectrometer used for?

Answer 42

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

Question 43

Use of mass spectrometer for identifying unknown compounds?

Answer 43

Chromatography- to detect banned drugs taken by athletes | Drug tests- drugs leave traces in the addict’s hair

Question 44

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

Answer 44

2,8, 8, 1

Question 45

Electronic configuration of Cr and Cu (odd ones out)

Answer 45

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)

Question 46

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

Answer 46

4s sublevel has less energy

Question 47

When are sublevels extra stable?

Answer 47

When they completely filled or half filled

Question 48

Ion

Answer 48

A charged atom (Has lost or gained electrons) Atom loses electrons—> positively charged Atom gains electrons—> negatively charged

Question 49

Reactivity of alkali metals...increases/decreases?

Answer 49

Very reactive (low first ionisation energy+a single electron in the outer energy level to be lost) Increases down the group (increasing atomic radius)