Chapter 1 - Atomic Structure

Question 1

how to change units

Answer 1

relate each to one metre
multiply by 10 to the … to get the larger unit into the lower unit
then compare

Question 2

letter symbol for atomic number

Answer 2

Z

Question 3

letter symbol for mass number

Answer 3

A

Question 4

what is the atomic number?

Answer 4

The number of protons in the nucleus of an atom for a specific element

Question 5

what is the mass number?

Answer 5

the number of protons plus the number of neutrons in an atom for a specific element

Question 6

what is an isotope?

Answer 6

Atoms of an element that contain a different number of neutrons

Question 7

when light is emitted, it is expressed as…

Answer 7

photons

Question 8

is light emitted when electrons absorb or lose energy

Answer 8

lose energy

Question 9

What is an isotopic symbol?

Answer 9

where a symbol of an element, the mass number and the atomic number are shown together. the mass number is above the atomic number with the element symbol nest to them

Question 10

when electrons absorb energy what happens?

Answer 10

They travel to a higher energy level. They jump levels in the electronic configuration

Question 11

what is an atomic emission spectrum?

Answer 11

a set of lines each representing different frequency of light, therefore each line corresponds to exactly one amount of energy being emitted

Question 12

what are the two elements with atypical configurations?

Answer 12

Chromium and Copper

Question 13

electrons/subshells are more stable when…

Answer 13

• all orbitals in a subshell are at least singly filled

- HUNDS RULE: subshells are either half or fully filled, orbitals are filled singularly before any are double filled.

Question 14

outline the bohr model

Answer 14

treats electrons as particles in fixed orbits travelling around the nucleus of an atom

Question 15

describe the quantum mechanical model

Answer 15

electrons are treated mathematically as a wave. proposed that within each shell there were several different energy levels called subshells. these subshells were where electrons could be found and different cloud shapes, thus, defeating the idea of fixed orbits.

Question 16

what is another name for the quantum mechanical model?

Answer 16

schrodinger’s model

Question 17

what atom model do we use today

Answer 17

the quantum mechanical model

Question 18

what were the negatives about bohrs model

Answer 18

referred to atoms as almost one dimensional in the sense that only one quantum number was used to describe the distribution of electrons.

bohrs model could not explain atomic emission spectrum more complex than hydrogen

Question 19

what were the positives about bohrs model

Answer 19

started to provide us with an understanding into the structure of the atom and also electronic configurations

Question 20

in the second shell there are…

Answer 20

2 subshells

Question 21

chromium configuraton

Answer 21

, 3p^6, 4s^1, 3d^5

Question 22

copper configuration

Answer 22

, 3p^6, 4s^1, 3d^10

Question 23

describe the electron arrangement in bohrs model

Answer 23

bohrs model used the 2n^2 rule to show how many electrons could fit in a shell. n represented the shell number e.g: shell 3 could fit 2 x 3^2 so 18 electrons

Question 24

how did the emission spectra help bohrs model

Answer 24

it helped bohrs model as it showed that only one line line was created for the emission spectra of hydrogen. it was then assumed that because there was only one shell in hydrogen this was the reason for the one lie on the spectrum. However, his model could not explain other elements emission spectra because his model did not depict multiple subshells within the shell.