Periodic Table

Question 1

What is a molecule

Answer 1

Two or more atoms bond by sharing electrons

Question 2

Compound

Answer 2

When atoms are from different elements

Question 3

Mass number

Answer 3

Number of protons-number of neutrons

Question 4

Neutrons

Answer 4

Mass number-atomic number

Question 5

Isotopes

Answer 5

Atoms of the same element can have different mass numbers. They have same atomic number but different number of Nuclei

Question 6

Maximum number of electrons for each shell

Answer 6

Shell1:2
Shell2:8
Shell3:18
Shell4:32

Question 7

Valence electrons

Answer 7

Electrons in the outermost shell of an atom

Question 8

Core charge formula

Answer 8

Number protons - inner shell electrons

Question 9

Atomic radius definition

Answer 9

Distance from Centre on atoms to valence electrons

Question 10

Electronegativity trends

Answer 10

High for non metals
Group 18 no electronegativity
Less pull when valence electrons further from nucleus

Question 11

First Ionisation energy

Answer 11

The energy required to remove first valence electron from atom

Question 12

First Ionisation Trends

Answer 12

Decreases going down a group
Increases across a period

Question 13

Metallic character

Answer 13

Easily lose electrons, conducts electricity and shiny

Question 14

Non- metallic character

Answer 14

Non- metals, gain electrons

Question 15

Metalloids

Answer 15

Mix of both metallic and non metallic

Question 16

Metallic trend

Answer 16

Going across a period decreasing metallic character

Question 17

What is reactivity

Answer 17

How easy it is for an atom to gain or lose electrons

Question 18

Reactivity trends

Answer 18

Group 1 most reactive followed by group 2 in the metals but in the non metals it’s group 17 followed by group 16
Group 18 no reactivity
Increase as you go up a group

Question 19

Atomic radii trends

Answer 19

Decrease from left to right across a period to group 18
Increase as you go down a group

Question 20

Electro negativity trends

Answer 20

Group 18 no electronegativity
Increase across a period and up a group

Question 21

why a neutral atom cannot have the atomic configuration of 6 protons, 13 neutrons and 13 electrons.

Answer 21

Neutral atoms must have the same number of protons (positively charged) and electrons (negatively charged). If a species had 6 protons and 13 electrons, it would have an overall charge of +7, which would make it a charged species (ion).

Question 22

Tellurium is element 52 and iodine is element 53. Explain why iodine atoms have less mass than tellurium atoms.

Answer 22

Tellurium atoms have more neutrons than iodine, resulting in a higher mass number and higher mass.

Question 23

what is an ion?

Answer 23

An atom or a molecule that has a positive or negative electrical charge. not neutral charge. (due to the loss or gain of one or more electrons.)

Question 24

Which of the following determines the chemical properties of an element?

Answer 24

The chemical properties of an element are determined by the electron configuration of its orbiting electrons as these interact with other atoms to form chemical bonds.

Question 25

How can the periodic table of the elements be used?

Answer 25

To predict how atoms of different elements will combine

Question 26

what is an atomic emission spectrum

Answer 26

the pattern of lines formed when light passes through a prism to separate it into the different frequencies of light it contains.

Question 27

Emission Spectrum definition

Answer 27

Light contains energy. If an atom has extra energy, it can get rid of it by sending out a little packet of light, called a photon. It also works the other way around: if a photon comes near an atom that could use some extra energy, the photon can be absorbed by the atom

Question 28

how many electrons can occupy subshells 1s 2s 2p 3s 3p 3d 4s 4p 4d 4f

Answer 28

1s=2 2s=2 2p=6 3s=2 3p=6 3d=10 4s=2 4p=6 4d=10 4f=14

Question 29

Energy consumption of absorption spectra and emission

Answer 29

An absorption spectrum is produced when atoms absorb energy. An emission spectrum is produced atoms release energy.

Question 30

Appearance of both spectras

Answer 30

Absorption spectra show dark lines or gaps Emission spectra show colored lines.

Question 31

Energy of an atom both spectrums

Answer 31

An atom obtains a higher energy level when an absorption spectrum is given by that atom. An emission spectrum is given when an excited atom obtains a lower energy level.