Chapter One: Atomic Structure

Question 1

Electron weight

Answer 1

1/1800 of a proton

Question 2

Are electrons and protons electrostatic?

Answer 2

Yes

Question 3

What is Bohr’s model?

Answer 3

Discovered in 1913 it is the structure that suggested that electrons orbited around the nucleus in definite paths called shells

Question 4

What is the most current model of the atom

Answer 4

Schrodinger

Question 5

Ion

Answer 5

An atom that has either lost or gained an electron

Question 6

Cation

Answer 6

Have lost electrons so they end up with a positive charge

Question 7

Anion

Answer 7

Gained electrons so they have a negative charge

Question 8

Macromolecules and examples

Answer 8

A very large molecule ie; synthetic polymers, proteins and DNA

Question 9

Nanometre

Answer 9

Is 1 billionth of a metre

Question 10

Conversion table

Answer 10

1m = 10^2cm = 10^3mm = 10^6micro = 10^9nm
1nm = 10^-9m = 10^-6cm

Question 11

What is nanotechnology?

Answer 11

Is working with technology at a nanoscale to create a cleaner, safer, longer lasting and smarter products for the future.

Question 12

What does nanoscience deal with?

Answer 12

Directly with atoms, molecules and macromolecules

Question 13

Energy properties

Answer 13

Energy is not continuous but comes in quanta and particles have wave properties.

Question 14

Quanta

Answer 14

Small packets of energy

Question 15

Molecular manufacturing

Answer 15

When scientists assemble materials atom by atom, to make atoms into specific molecules and create a specific product.

Question 16

Isotope

Answer 16

Atoms of the same element that have different numbers of neutrons

Question 17

Isotope properties

Answer 17

Have similar chemical properties due to electron structure

Have different physical properties due to their different masses

Question 18

Aufbau’s rule

Answer 18

In ground state electrons fill orbitals of lowest energy level before occupying higher energy levels.

Question 19

Ground state

Answer 19

Electrons are in their most stable configuration

Question 20

Hund’s rule

Answer 20

Every orbital in a subshell is singly occupied with one electron before any one orbital is doubly occupied.

Question 21

Filling subshells rule

Answer 21

Fully filled subshells are more stable than half filled subshells which are more stable than partially filled subshells

Question 22

What causes colour in fire?

Answer 22

Is the way the electrons are arranged around the nucleus of an atom

Question 23

What does arrangement of electrons determine?

Answer 23

The properties and behaviour of elements and the materials made from them

Question 24

What happens when a white light is passed trhough a prism?

Answer 24

It creates a continuous spectrum of colour

Question 25

Why does an element emit light when heated?

Answer 25

Becuase the atoms absorb energy then when they return to ground state they release the energy as light.

Question 26

How do you create an emission spectrum

Answer 26

By passing the light emitted by an element through a prism.

Question 27

What does an emission spectrum show?

Answer 27

The lines correspond to the energy difference between electron shell levels

Question 28

What is the difference between a continuous spectrum and the emission spectrum?

Answer 28

The continuous spectrum is formed when a light is passed through a prism whereas the emission spectrum is the light emitted from an element that has been passed through a prism.

Question 29

Excited electrons in Bohr’s model

Answer 29

In Bohr’s model the electron float around an orbit of the nucleus in their specific energy levels, then they jump from their ground state up to the next shell and when they return the energy released is produced as light

Question 30

How can you identify an element based on the light it releases?

Answer 30

Because there are only specific energy levels released they correspond to a line on the emission spectrum.

Question 31

Shells capacity

Answer 31

2n^2 (n is the shell)

The outer shell never has more than 8 electrons in the first 20 elements

Question 32

What are the limitations of Bohr’s model?

Answer 32

The electrons don’t actually travel in paths

The filling order has exceptions

Question 33

When and who discovered the quantum theory?

Answer 33

Erwin Schrodinger in 1926

Question 34

What is the Quantum Mechanical Model?

Answer 34

Is a complex mathematical model based on particles such as electrons showing wave like behaviour

Question 35

What makes up the Quantum Mechanical Model?

Answer 35

Shells, subshells and orbitals

Question 36

Shells

Answer 36

Shell 2, shell 3 etc

Question 37

Subshells

Answer 37

s,p,d,f

Shell 2 = 2 subshells

Question 38

Orbitals

Answer 38

What make up the subshells

Question 39

Plum pudding model

Answer 39

Sir J.J Thompson suggested that an atom is a positively charged sphere that had electrons embedded in the sphere discovered in 1897

Question 40

Subatomic particles

Answer 40

Electrons
Neutrons
Protons

Question 41

Molecules

Answer 41

Are substances that consist of 2 or more atoms chemically combined
The types of atoms, size, arrangement and shape significantly impact the properties of materials

Question 42

Potential risks of nanotechnology

Answer 42

Miniaturised weapons

Designing biological organisms

Question 43

Excited states

Answer 43

When an atom moves to a higher energy level than the ground state by absorbing energy
The outermost energy electron moves to a higher subshell

Question 44

Exceptions to the filling rule

Answer 44

Chromium 24 and copper 29
chromium fills to 3d^5
copper fills to 3d^10

Question 45

Stability of shells

Answer 45

Filled shells are more stable than half filled shells which are more stable than partially filled shells

Question 46

Schrodinger’s model

Answer 46

Proposed that electrons would move around in regions of space called orbitals

Question 47

Max. electrons a subshell can hold

Answer 47

s - 2
p - 6
d - 10
f - 14

Question 48

How many electrons in an orbital?

Answer 48

0, 1 or 2