Textboolk LO1-3

Question 1

Quantization

Answer 1

Only certain energies are allowed

Question 2

Principle quantum number (2)

Answer 2

A positive unit less integer
defines the energy of the allowed orbits in the H atom

Question 3

The energy of the electron in an orbit has a negative value because

Answer 3

the electron in the atom has a lower energy than when it is free.

Question 4

The 0 of energy occurs when

Answer 4

n= infinity
That is when the election is infinitely separated from the nucleus

Question 5

Ground state

Answer 5

An atom with its electron in the lowest possible energy levels

Question 6

The energy of the electron depends on

Answer 6

n

Question 7

The larger the value of n, (radius and energy negativity)

Answer 7

The larger the Bohr radius and the less negative the value of the energy

Question 8

The difference between successive energy levels becomes _________ because

Answer 8

smaller as n becomes larger

Energy is dependent on 1/n^2

Question 9

what needs to happen when an electron goes From n=1 to n=2 electron state

Answer 9

Energy is absorbed from the surroundings

Question 10

A consequence or requirement of quantization (2)

Answer 10

A specific and precise amount of energy

No more or no less

Question 11

When a electron falls down its energy level to a diff one

Answer 11

Since only certain energy levels are possible, only photons with particular energies and wavelengths are emitted

Question 12

principle quantum number (3)

Answer 12

any integer from 1-infinity

primary factor in determining the energy of an orbital
defines size of an orbital

Question 13

In atoms having more than 1 electron, two or more electrons may have the same n value. They are said to be

Answer 13

in the same electron shell

Question 14

orbital example

Answer 14

3px

Question 15

which quantum number or combination is needed to specify a given subshell in an atom?

Answer 15

n and l

Question 16

repulsion counteract the nuclear attraction making electrons

Answer 16

easier to remove by helping to push it away

Question 17

shielding reduces the full nuclear charge to

Answer 17

an effective nuclear charge

Question 18

the energy difference arises from three factors

Answer 18

nuclear attractions, electron repulsion and orbital shape

Question 19

puli exclusion principle

Answer 19

requires each electron to have a unique set of four quantum number

Question 20

repulsion shield electrons from the ______ reducing it to an_____

Answer 20

the full nuclear charge

effective nuclear charge

Question 21

aufbau principle

Answer 21

we start at the beginning of the periodic table and add one proton to the nucleus and one electron to the lowest energy sub level available.

Question 22

order for filling energy sub levels

Answer 22

1s, 2s, 2p,3s,3p,4s,3d,4p,5s,4d,5p

Question 23

Hunds rule

Answer 23

No electrons are paired in a set of orbitals of equal energy until every orbital in the set has one electron.

Question 24

formula for which orbital filled first

Answer 24

n+l

Whichever orbital has the lower n+1 value will fill first

Question 25

formula for maximum electron possible for nth shell

Answer 25

2n^2

Question 26

the energy gaps between sub shells of a given shell becomes______ as n _____

Answer 26

smaller increase

Question 27

The electrons included in the noble gas notation are often referred to as

Answer 27

core electrons

Question 28

What are the two exceptions for transition metals and draw it out

Answer 28

Question 29

Transition metal steps or exceptions for electron configs

Answer 29

Make sure that d orbital is half filled (5) or fully filled (10) by promoting electrons from the 4s

Question 30

from Scandium and onwards, the 3d orbital of transition metals actually becomes

Answer 30

lower in energy than the 4s, which is why we write 3d before 4s in the configuration.