Chapter 2- Elements Of The Periodic Table

Question 1

What do atoms make up

Answer 1

all matter

Question 2

What are atoms composed of

Answer 2

Protons, neutrons, electrons

Question 3

What is mass of atom determined by

Answer 3

Mostly mass of nucleus

Question 4

What is diameter of atom determined by

Answer 4

Cloud of electrons

Question 5

Protons are

Answer 5

Positively charged

Question 6

Neutrons are

Answer 6

Neutral

Question 7

Electrons are

Answer 7

Negatively charged

Question 8

Where are protons and neutrons found

Answer 8

In the nucleus

Question 9

Where are electrons found

Answer 9

Outside of the nucleus

Question 10

The charges of protons and electrons are

Answer 10

Equal but opposite

Question 11

What does an element contain

Answer 11

Atoms of the same type

Question 12

How can you find the number of protons/ electrons in an element

Answer 12

The atomic number

Question 13

A-Z=

Answer 13

Number of neutrons

Question 14

What are isotopes

Answer 14

Atoms with the same atomic number but different mass numbers

Question 15

What are ions

Answer 15

Atoms that have lost or gained electrons to become charged particles

Question 16

What is the emission spectra

Answer 16

When atoms are heated, they can emit electromagnetic radiation in the form of coloured light. When light is passed through a prism it produces a spectrum made up of lines of different colours

Question 17

What is the Bohr model

Answer 17

The first atomic model to explain origin of emission spectra

Question 18

What does the Bohr model assume

Answer 18

Electrons only exist in fixed, circular orbits if specific energies which later came to be known as energy levels or shells

Question 19

What does each line in the emission spectrum correspond to

Answer 19

A specific electron transition between shells

Question 20

How to calculate how many electrons each shell can hold

Answer 20

2n(squared)

Question 21

How many electrons can the valance shell contain

Answer 21

No more than eight

Question 22

What is oxidation

Answer 22

Additional of oxygen to a substance or removal of hydrogen from a substsnce

Question 23

What is the octet rule

Answer 23

atoms will lose, gain or share electrons so that they can achieve 8 valence electrons as this is stable

Question 24

What are the limitations of the Bohr model

Answer 24

1- no reason why a shell like the 3d would only fill up to 8.
2- cannot predict emission spectra of elements with more than one electron
3- is unable to explain why shells hold 2n(squared) electrons

Question 25

What does the Schrodinger model suggest

Answer 25

electron shells are further divided into subshells

Question 26

what are the subshells labelled as

Answer 26

s,p,d,f

Question 27

What are orbitals

Answer 27

subshells are split into orbitals

Question 28

how many electrons can an orbital hold

Answer 28

2 electrons

Question 29

how many subshells does the first shell have (labelled)

Answer 29

1 (s)

Question 30

how many subshells does the second shell have (labelled)

Answer 30

2 (s, p)

Question 31

how many subshells does the third shell have (labelled)

Answer 31

3 (s, p, d)

Question 32

what is the max electrons shell 1 can have

Answer 32

2

Question 33

what is the max electrons shell 2 can have

Answer 33

8

Question 34

what is the max electrons shell 3 can have

Answer 34

18

Question 35

how many orbitals does the s subshell have

Answer 35

1

Question 36

how many orbitals does the p subshell have

Answer 36

3

Question 37

how many orbitals does the d subshell have

Answer 37

5

Question 38

What is a ground state of an atom

Answer 38

has the electrons in the lowest possible energy subshells

Question 39

What happens if an atom is in an excited state

Answer 39

when if energy is supplied to the atom, one or more of the outer electrons can jump into the next subshell

Question 40

What are the exceptions for subshell configuration

Answer 40

Chromium and Copper

Question 41

what do horizontal rows of the period table represent

Answer 41

periods labelled 1-7

Question 42

what do vertical columns of the periodic table represent

Answer 42

groups, labelled 1-8

Question 43

what do valence electrons give their elements

Answer 43

chemical properties

Question 44

what are critical elements

Answer 44

elements that exist in small quantities and are rare and endangered, heavily relied on for industry and the running of society.

Question 45

what is core charge

Answer 45

the attraction of the nucleus with the outer shell electrons

Question 46

what is the pattern of atomic radii

Answer 46

atoms get bigger as we move down a group (because extra shells are used), and they get smaller from left to right (because of core charge)

Question 47

how to determine nuclear charge

Answer 47

core charge= # of protons - # of inner shell electrons

Question 48

what is the pattern of reactivity

Answer 48

as you go down a group of metals they get more reactive (as its easier to lose electrons)
as you go down a group of non-metals they get less reactive (as its easier to gain electrons)

Question 49

what is electronegativity

Answer 49

the ability of an atom to attract electrons

Question 50

what is first ionization energy

Answer 50

the amount of energy required to remove 1 electron from an atom.

Question 51

what is the pattern of first ionization energy

Answer 51

as you go down a group the energy level decreases (due to core charge remaining the same)
left to right it increases (core charge increases and therefore electrons are attracted more to the nucleus)