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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?

25
How is electron affinity different to ionisation?
- ionisation energies are always concerned with the formation of positive ions whereas electron affinities are the negative ion equivalent
26
What is electron affinity?
energy released to attach one electron to atoms (electron is fully detached from another one and electron transfer occurs)
27
What are teh differences between electronegativity and electron affinity?
= 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
When are compounds formed?
Compounds are formed when elements share or transfer electrons to achieve a full outer
29
What is the behaviour/reactivity of an atom determined by?
Outer shell valence electrons
30
Define a chemical bond
A link between atoms and molecules
31
What types of bond exist? (4)
- ionic, covalent and metallic - intermolecular forces - free radicals - complexes and chelates
32
What is a free radical?
An atom that has at least one unpaired electron and is therefore unstable and highly reactive
33
Describe the electronegativity trend in the periodic table
``` it increases horizontally (left to right) decreases vertically (top to bottom) ```
34
When do mainly ionic bonds form?
When atoms have a large difference in electronegativity
35
When do mainly covalent bonds form?
when atoms have very similar electronegativity; sharing of electrons
36
If the EN is greater than 2.0 the bond is ___
ionic
37
If the EN is between 0.5 and 1.6 the bond is ___
covalent
38
if the EN is less than 0.5 the bond is ___
Nonpolar covalent
39
If it is between 1.6 and 2.0 (and if a metal is involved), then the bond is ___
Ionic
40
If it is between 1.6 and 2.0 (and only non-metals are involved), then the bond is ___
Polar covalent
41
What does the chemical formulae tell us?
1. The elements that are present in a substance | 2. The relative number of atoms that make up that substance
42
What is valency?
Combining power of an atom
43
Explain the octet rule
most stable configuration is when the outer shells are fully filled where 8 electrons in the outer shell.
44
What is ionic bonding?
an electrostatic attraction between ions with opposite charges
45
When does an ionic bond occur?
When a metal is large with low ionisation energy and a non metal is small with high electron affinity
46
When is the attractive force of an ionic bond maximised?
When an ion is surrounded by a lattice of oppositely charged ions
47
Name some properties of ionic compounds (4)
- conduct electricity - high melting and boiling points - hard solids - form crystalline structures]
48
Name some properties of covalent compounds
- lower melting points and boiling points than ionic compounds - low solubility - poor electrical conductivity
49
What is a polar molecule?
When a molecule has a slightly positive end and a slightly negative end
50
When does metallic bonding occur?
When the outer electrons from the metal atoms merge to produce a lattice of negative metal ions in a sea of delocalised electrons
51
What does the strength of the metal depend on?
- the charge and the size of the metal ion
52
How can metals conduct electricity?
They have a sea of delocalised electrons which can move through the structure to carry the charge
53
Why do transition metals tend to have particularly high melting and boiling points?
- they can involve the 3d electrons in the delocalisation as well as the 4s
54
Why is Fe 3+ more stable than Fe2+?
Because Fe3+ has a half filled outer orbital
55
Where do electrons fill up in an atom first?
the low energy orbitals, closer to the nucleus
56
For d block elements (transition metals) what electrons are lost first during ionisation?
4s electrons are lost first because they have a higher energy level than 3d
57
Name the reactivity properties of Group 1 alkaline metals
- form oxides which dissolve in water to form alkaline solution - readily lose electrons to form +1 ionic compounds
58
Name the reactivity properties of Group 2 alkaline metals
- 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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