Brainscape's Knowledge GenomeTM

Browse over 1 million classes created by top students, professors, publishers, and experts.


See full index

AH Chemistry (short) > Unit 1- Inorganic chemistry > Flashcards

Unit 1- Inorganic chemistry Flashcards

You may prefer our related Brainscape-certified flashcards:
Periodic Table flashcards Chemistry 101 flashcards AP® Chemistry flashcards Organic Chemistry 101 flashcards
1
Q

A photon carries energy proportional to what?

A

The frequency of radiation

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
2
Q

The photons in which frequency of radiation can transfer greater amounts of energy?

A

Those in high frequency radiation transfer greater amounts of energy

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q

What can happen to the electrons within atoms when energy is transferred to these atoms?

A

The electrons can be promoted to higher energy levels

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
4
Q

When does an atom emit a photon of light energy?

A

When an excited electron moves from a higher energy level to a lower energy level

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
5
Q

What happens in absorption spectroscopy?

A

Electromagnetic radiation is directed at an atomised sample, the radiation is then absorbed as electrons are promoted to higher energy levels

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
6
Q

What happens in emission spectroscopy?

A

High temperatures are used to excite the electrons within atoms, as the electrons drop to lower energy levels, photons are emitted

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
7
Q

In atomic spectroscopy, what is the concentration of the element within a sample related to?

A

The intensity of light emitted or absorbed

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
8
Q

What are the 4 different shapes of orbitals?

A

s, p, d and f

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
9
Q

How do electrons behave in an atom?

A

As standing waves. These are waves that vibrate in time but do not move in space. There are different sizes and shapes of standing wave possible around the nucleus, known as orbitals

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

How many electrons can an orbital hold?

A

A maximum of 2

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
11
Q

How many electrons can an orbital hold?

A

A maximum of 2

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
12
Q

What is the order of the electromagnetic spectrum from highest to lowest energy?

A

Gamma rays, X-rays, ultraviolet, visible light, infrared, microwaves and radio waves

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
13
Q

Electrons within atoms have fixed amounts of energy called…?

A

Quanta

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
14
Q

It is possible to describe any electron within an atom using four quantum numbers, what are these and what do they tell us about the electron?

A
  • principal quantum number (n)- indicates the main energy level for an electron and is related to the size of the orbital
  • angular momentum number (l)- determines the shape of the subshell and can have values from zero to n-1
  • magnetic quantum number (m)- determines the orientation of the orbital and can have values between -l and +l
  • spin magnetic quantum number (s)- determines the spin and can have values of +1/2 or -1/2
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
15
Q

What are the 3 rules that determine how electrons within atoms are arranged?

A
  • the aufbau principle
  • Hund’s rule
  • the Pauli exclusion principle
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
16
Q

What is the aufbau principle?

A

Electrons fill orbitals in order of increasing energy

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
17
Q

What is Hund’s rule?

A

When degenerate orbitals are available, electrons fill each singly, keeping their spins parallel before spin pairing starts

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
18
Q

What is the Pauli exclusion principle?

A

No two electrons in one atom can have the same set of 4 quantum numbers, therefore, no orbital can hold more than two electrons and these two electrons must have opposite spins

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
19
Q

In an isolated atom, what can be said about the orbitals within each subset?

A

They are degenerate (have the same energy)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
20
Q

The periodic table can be split into 4 blocks (s, p, d and f), which correspond to what?

A

The outer electronic configuration of the elements within these blocks

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
21
Q

How are electron pairs arranged?

A

To minimise repulsion and maximise separation

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
22
Q

What are the names for the arrangement of electron pairs around a central atom for two through to six electron pairs?

A 
two electron pairs= linear
three electron pairs= trigonal planar
four electron pairs= tetrahedral
five electron pairs= trigonal bipyramidal
six electron pairs= octahedral
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
23
Q

What is the order of electron pair repulsions in order from most repulsion to least repulsion?

A
  • bonded pair/bonded pair (most repulsion)
  • non-bonded pair/bonded pair
  • non-bonded pair/non-bonded pair (least repulsion)
24
Q

What are the d-block transition metals?

A

Metals with an incomplete d subshell in at least one of their ions

25
Q

The filling of d orbitals follows the aufbau principle, with the exception of which two elements and why is this?

A

Chromium and copper, these exceptions are due to the special stability associated with the d subshell being half filled or completely filled

26
Q

When atoms from the first row of the transition elements form ions, what electrons do they lose first?

A

The 4s electrons are lost first rather than the 3d electrons

27
Q

What oxidation number do uncombined elements have?

A

zero

28
Q

What is the oxidation number of ions containing single atoms?

A

The oxidation number is the same as the charge on the ion

29
Q

In most of its compounds, what is oxygen’s oxidation number?

A

-2

30
Q

In most of its compounds, what is hydrogen’s oxidation number?

A

+1

31
Q

What must the sum of all the oxidation numbers in a neutral compound add up to?

A

zero

32
Q

What must the sum of all the oxidation numbers in a polyatomic ion add be equal to?

A

The charge on the ion

33
Q

What can oxidation be defined as?

A

An increase in the oxidation number

34
Q

What can reduction be defined as?

A

A decrease in the oxidation number

35
Q

What are oxidising agents often?

A

Compounds containing metals in high oxidation states

36
Q

What are reducing agents often?

A

Compounds containing metals in low oxidation states

37
Q

What are ligands?

A

Negative ions or molecules with non-bonding pairs of electrons that they donate to the central metal atom or ion, forming dative covalent bonds

38
Q

What is a dative covalent bond?

A

a covalent bond (a shared pair of electrons) in which both electrons come from the same atom

39
Q

What are the classifications of ligands and give examples of each?

A
  • monodentate (NH3, Cl-)
  • bidenatate (oxalate ion)
  • hexadentate (EDTA)
40
Q

What is the coordination number of a ligand?

A

The total number of bonds from the ligands to the central transition metal

41
Q

What can be said about the d orbitals in a complex of a transition metal?

A

They are no longer degenerate

42
Q

When does the splitting of d orbitals to higher and lower energies occur?

A

When the electrons present in approaching ligands cause the electrons in the orbitals lying along the axes to be repelled

43
Q

What is the difference between strong and weak field ligands?

A

Strong field ligands cause a large difference in energy between subsets of d orbitals, weak field ligands cause a small energy difference

44
Q

What are heterogeneous catalysts?

A

Catalysts which are in a different state to the reactants

45
Q

What are homogeneous catalysts?

A

Catalysts which are in the same state as the reactants

46
Q

Why is electromagnetic radiation said to have a dual nature?

A

Because it can be described as both a wave and a particle

47
Q

What are photons?

A

When electromagnetic radiation is absorbed or emitted by matter it behaves like a stream of particles. These particles are known as photons

48
Q

What can be used to identify an element?

A

It’s characteristic emission and absorption spectra

49
Q

How can the discrete lines observed in atomic spectra be explained?

A

If electrons, like photons also display the properties of both particles and waves

50
Q

What shape are S orbitals?

A

Spherical

51
Q

What 2 elements are not transition metals when they would be expected to be and why?

A

Zinc and scandium, they are not transition metals as they do no form a stable lot

52
Q

What can be said about compounds of the same transition metal in different oxidation states?

A

They may have different colours

53
Q

What is a transition metal complex?

A

A compound made of a transition metal ion covalently bonded to ligands

54
Q

What is the spectrochemical series?

A

The order that ligands can be placed in based on their ability to split d orbitals

55
Q

What are the 3 main indicators of a transition metal?

A
  1. Can produce ions with different valencies
  2. Make coloured compounds
  3. Have catalytic uses

AH Chemistry (short) (4 decks)

Brainscape helps you reach your goals faster, through stronger study habits.
© 2024 Bold Learning Solutions. Terms and Conditions