3) Atomic Structure

Question 1

Nucleus

Answer 1

the positively charged center of the atom consisting of protons and neutrons

Question 2

Electron cloud model

Answer 2

says that we cannot know exactly where an electron is at any given time, but the electrons are more likely to be in specific areas. These areas are specified by orbitals. The orbitals are specified by shells and sub-orbitals

Question 3

Electron

Answer 3

Extremely small negatively charged subatomic particle with a mass of approx. one two-thousandth the mass of a hydrogen atom

Question 4

Proton

Answer 4

Small positively charged subatomic particle having a mass approx. equal to the mass of a hydrogen atom and a charge equal in magnitude (but opposite in sign) to an electron

Question 5

Neutron

Answer 5

A small neutral subatomic particle that has the same mass as a proton

Question 6

Atomic number (Z)

Answer 6

number of protons in the nucleus of an atom of that element

Question 7

Mass number (A) [nucleon number]

Answer 7

number of protons plus neutrons in the nucleus of an atom of the species concerned

Question 8

Nucleon

Answer 8

A term sometimes used to describe a proton or neutron

Question 9

Isotopes

Answer 9

• atoms with same number of protons but different numbers of neutrons
• have the same atomic number but different mass numbers (named by mass number)

Question 10

Relative abundance of an isotope

Answer 10

percentage of that isotope in the naturally occurring element

Question 11

Why e- not attracted to nucleus (usually positives/negatives attract)

Answer 11

Electrons possess energy sufficient to resist the attraction towards the positive nucleus

Question 12

What did Niels Bohr do

Answer 12

1913: first person to develop a theory to explain the arrangement of electrons in atoms

Question 13

Bohr theory

Answer 13

Bohr model: proposed that the electrons in an atom exist in fixed energy levels (shells), called the first, second, third energy level, and so on.. (energy increases as shells increase)

Question 14

Electron configuration

Answer 14

the arrangement of electrons in any given atom - determined by allocating the electrons to the energy levels, starting at the lowest

Question 15

Why do noble gases tend not to undergo chemical reaction

Answer 15

Energy levels filled to eight electrons - meaning the electron configuration is stable

Question 16

What is the ‘driving force’ behind chemical reactivity

Answer 16

An atom tends to lose, gain, or share electrons to move towards a more stable and lower-energy state

Question 17

Valence electrons

Answer 17

electrons in the highest energy level (outermost energy shell)

Question 18

Valence shell

Answer 18

the outermost energy level

Question 19

Transition elements (transition metals)

Answer 19

result from converting a semi-filled energy level with eight electrons to a completely filled energy level with 18 electrons. The transition elements are groups 3 - 12

Question 20

Orbital

Answer 20

Volume of space surrounding the nucleus of an atom where one or two electrons may randomly move

Question 21

What is the max amount of electrons each orbital can accomodate

Answer 21

2

Question 22

Energy sublevels

Answer 22

regions within an atom’s energy levels (or shells) that are further divided based on the shape and energy of the orbitals and are denoted by the letters s, p, d, and f

Question 23

Colour of LITHIUM in a flame test

Answer 23

carmine (dull red)

Question 24

Colour of SODIUM in a flame test

Answer 24

yellow

Question 25

Colour of POTASSIUM in a flame test

Answer 25

light purple (lilac)

Question 26

Colour of CALCIUM in a flame test

Answer 26

brick-red (orange-red)

Question 27

Colour of STRONTIUM in a flame test

Answer 27

scarlet (deep red)

Question 28

Colour of BARIUM in a flame test

Answer 28

pale green (apple green)

Question 29

Colour of COPPER in a flame test

Answer 29

blue-green

Question 30

When burning elements, what gives the flame its distinctive colour?

Answer 30

High temp decomposes compound into elements, and elements give colour

Question 31

Bohr theory (1913)

Answer 31

Electrons move around the nucleus in fixed orbits. When they absorb energy, they move to orbits of larger radius, and if they emit energy (as light) they fall back to the smaller orbit

Question 32

Planck's quantum theory

Answer 32

In atoms, energy does not vary but exists in fixed packages

Question 33

Schrodinger equation

Answer 33

Uses wave properties and quantum theory to calculate probability of finding an electron at a specific location

Question 34

Orbitals (letters & numbers)

Answer 34

s (starts at 1), p (starts at 2), d (starts at 3), f (starts at 4)