Topic test, Atomic theory

Question 1

Nanoscale

Answer 1

used to describe objects that are 1-100nm wide

Question 2

surface area to volume ratio features

Answer 2

• transport chemicals more effectively
• absorb unwanted chemicals more easily
• effective catalysts as they allow reactant molecules to come in contact with each other to form new substances

Question 3

Elements

Answer 3

One type of atom that cannot be broken down anymore

Question 4

Compounds

Answer 4

Different types of atoms that combine to form new substances

Question 5

atoms

Answer 5

the building blocks of all matter

Question 6

subatomic particles

Answer 6

the sub particles in atoms

Question 7

monatomic

Answer 7

elements made of only one atom (full shell elements)

Question 8

Isotopes

Answer 8

atoms that have the same number of protons but different number of neutrons

Question 9

Bohr model

Answer 9

shows probability clouds that show where an electron could be at any given moment

Question 10

sub shells

Answer 10

shells contain separate energy levels of similar energy

Question 11

orbitals

Answer 11

Each subshell is made up of smaller components known as orbitals

Question 12

sub shell notation

Answer 12

1s<2s<2p<3s<3p<4s<3d<4p<5s<4d<5p<6s<4f<5d

Question 13

chromium and copper sub shell notation

Answer 13

an exception, scientist have found filling the “3d” shell and removing one electron from the 4s shell is more stable

Question 14

Periodicity

Answer 14

Periodicity shows the variation across periods and similarity down groups for electrons. recurring variations in element properties with increasing atomic number.

Question 15

atomic number patterns

Answer 15

increases both across a period and down a group. As protons and electrons are added, atomic number increases

Question 16

atomic size patterns

Answer 16

across a period decreases - more electrons increases the electrostatic attraction and the radius is decreased
down a group increases- there are more shells so the size is larger

Question 17

electronegativity patterns

Answer 17

the ability of an atom to attract external electrons.
across a period- generally increases- the smaller the atomic radius the less electrons there are to block the attraction of the protons in the nucleus.
Down a group it decreases

Question 18

Core charge

Answer 18

is the measure of the attractive force felt by the valence shell electrons towards to nucleus.
core charge = number of protons - total number of electrons in full shells
Down a group core charge stays the same as the number of valence electrons also stays the same
as core charge increases, so does electronegativity

Question 19

first ionisation energy

Answer 19

the energy to remove one electron from an atom of an element in the gas phase
across a period (increases, harder to remove electron)- the smaller atomic size, the stronger the core charge making it harder to remove an electron
Down a group decreases- as more shells are added, core charge decreases so the electrons are easier to remove

Question 20

Metallic character

Answer 20

across a period decreases

down a group increases

Question 21

non metallic character

Answer 21

across a period increases

down a group decreases

Question 22

cation size

Answer 22

cations are smaller because they have lost their valence electrons which means the have lost it’s outer shell

Question 23

Anion size

Answer 23

Larger because they are have gained valence electrons