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Molcules and Materials- First year uni > Atoms and periodic table > Flashcards

Atoms and periodic table Flashcards

1
Q

How are organic molecules defined?

A

Due to carbon ring present

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2
Q

What is the difference between energy and matter?

A

Matter; form and mass

Energy; ability to do work

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3
Q

Name the 3 particles found inside an atom and their charges

A

Proton (+ve)
Neutron (NO charge)
Electron (-ve)

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4
Q

What components of an atom have mass or energy?

A

Protons and neutrons have mass

Electrons have energy

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5
Q

Define atomic number

A

The charge in the nucleus, no. of protons/ electrons

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6
Q

Define atomic mass

A

No. protons + no. neutrons

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7
Q

What does the arrangement of electrons in an atom determine?

A

The element’s stability and reactivity

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8
Q

What is an atomic orbital?

A

The region we can find electrons with a high probability

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9
Q

How many electrons can one orbital hold up to?

A

Up to 2 electrons

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10
Q

How is electronic configuration written out?

A

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

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11
Q

What does it mean if the outer shell of an atom is full?

A

They are stable and unreactive

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12
Q

Describe the periodic table trends in vertical groups and horizontal groups?

A

vertical groups = elements with similar properties

Horizontal groups = correspond to trends in behaviour

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13
Q

What is ionisation?

A

The process of removing electrons from an atom,

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14
Q

Describe what is meant by ‘the first ionisation energy’

A

the minimum energy needed to completely remove the most easily removed electron from the attraction of the atomic nucleus.

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15
Q

What does a high ionisation value show?

A

A high attraction between the electron and the nucleus

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16
Q

What factors affect the size of attraction of an ionisation energy?

A
  • charge on the nucleus
  • distance of electron from the nucleus
  • the no. electrons between the outer electrons and nucleus
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17
Q

Name the title of elements found in group 1 and 2 on the periodic table

A

alkaline metals

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18
Q

Name a few characteristics of transition metals

A
  • lower reactivity
  • multiple oxidation states
  • key to biological processes
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19
Q

Name the title of elements found in group 3 and 4 on the periodic table

A

Metalloids

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20
Q

Name the title of elements found in group 7 on the periodic table

A

Halogens

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21
Q

Name the title of elements found in group 8 on the periodic table

A

Noble gases

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22
Q

What are some features of noble gases?

A

Very stable due to full outer shells and therefore very unreactive and difficult to form compounds

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23
Q

Define electronegativity

A

ability of an atom within an molecule to attract electrons

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24
Q

Where are the most electronegative elements found on the periodic table?

A

Top right

25
Q

How is electron affinity different to ionisation?

A
  • ionisation energies are always concerned with the formation of positive ions whereas electron affinities are the negative ion equivalent
26
Q

What is electron affinity?

A

energy released to attach one electron to atoms (electron is fully detached from another one and electron transfer occurs)

27
Q

What are teh differences between electronegativity and electron affinity?

A

= Electron affinity is a property of individual atom, electronegativity is a property of an atom in a molecular
= Electron affinity is a fixed and truly measured value; electronegativity is non-measurable, and variable in different chemical environment
= Electron affinity is the energy released to attach on electron to atoms (electrons is fully detached from another atom, and electron -transfer happen
whereas electronegativity is the tendency to attract one electron to form a covalent bond

28
Q

When are compounds formed?

A

Compounds are formed when elements share or transfer electrons to achieve a full outer

29
Q

What is the behaviour/reactivity of an atom determined by?

A

Outer shell valence electrons

30
Q

Define a chemical bond

A

A link between atoms and molecules

31
Q

What types of bond exist? (4)

A
  • ionic, covalent and metallic
  • intermolecular forces
  • free radicals
  • complexes and chelates
32
Q

What is a free radical?

A

An atom that has at least one unpaired electron and is therefore unstable and highly reactive

33
Q

Describe the electronegativity trend in the periodic table

A 
it increases horizontally (left to right)
decreases vertically (top to bottom)
34
Q

When do mainly ionic bonds form?

A

When atoms have a large difference in electronegativity

35
Q

When do mainly covalent bonds form?

A

when atoms have very similar electronegativity; sharing of electrons

36
Q

If the EN is greater than 2.0 the bond is ___

A

ionic

37
Q

If the EN is between 0.5 and 1.6 the bond is ___

A

covalent

38
Q

if the EN is less than 0.5 the bond is ___

A

Nonpolar covalent

39
Q

If it is between 1.6 and 2.0 (and if a metal is involved), then the bond is ___

A

Ionic

40
Q

If it is between 1.6 and 2.0 (and only non-metals are involved), then the bond is ___

A

Polar covalent

41
Q

What does the chemical formulae tell us?

A
  1. The elements that are present in a substance

2. The relative number of atoms that make up that substance

42
Q

What is valency?

A

Combining power of an atom

43
Q

Explain the octet rule

A

most stable configuration is when the outer shells are fully filled where 8 electrons in the outer shell.

44
Q

What is ionic bonding?

A

an electrostatic attraction between ions with opposite charges

45
Q

When does an ionic bond occur?

A

When a metal is large with low ionisation energy and a non metal is small with high electron affinity

46
Q

When is the attractive force of an ionic bond maximised?

A

When an ion is surrounded by a lattice of oppositely charged ions

47
Q

Name some properties of ionic compounds (4)

A
  • conduct electricity
  • high melting and boiling points
  • hard solids
  • form crystalline structures]
48
Q

Name some properties of covalent compounds

A
  • lower melting points and boiling points than ionic compounds
  • low solubility
  • poor electrical conductivity
49
Q

What is a polar molecule?

A

When a molecule has a slightly positive end and a slightly negative end

50
Q

When does metallic bonding occur?

A

When the outer electrons from the metal atoms merge to produce a lattice of negative metal ions in a sea of delocalised electrons

51
Q

What does the strength of the metal depend on?

A
  • the charge and the size of the metal ion
52
Q

How can metals conduct electricity?

A

They have a sea of delocalised electrons which can move through the structure to carry the charge

53
Q

Why do transition metals tend to have particularly high melting and boiling points?

A
  • they can involve the 3d electrons in the delocalisation as well as the 4s
54
Q

Why is Fe 3+ more stable than Fe2+?

A

Because Fe3+ has a half filled outer orbital

55
Q

Where do electrons fill up in an atom first?

A

the low energy orbitals, closer to the nucleus

56
Q

For d block elements (transition metals) what electrons are lost first during ionisation?

A

4s electrons are lost first because they have a higher energy level than 3d

57
Q

Name the reactivity properties of Group 1 alkaline metals

A
  • form oxides which dissolve in water to form alkaline solution
  • readily lose electrons to form +1 ionic compounds
58
Q

Name the reactivity properties of Group 2 alkaline metals

A
  • form insoluble oxides found in ground deposits

- readily lose 2 electrons to form +2 ionic compounds

Molcules and Materials- First year uni (13 decks)

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