Brainscape's Knowledge GenomeTM


Top Flashcards (Certified)
All Flashcards

Z. Hchem > Unit 1 > Flashcards

Unit 1 Flashcards

(68 cards)

Start Studying
1
Q

How are elements on the periodic table arranged?

A

Elements on the periodic table are arranged by increasing atomic number.

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

What does the position of elements on the periodic table allow us to predict?

A

The position of elements on the periodic table allow chemists to make predictions of their physical properties and chemical behaviour.

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

What happens as you go down a group in the periodic table regarding electrons?

A

Going down in a group on the periodic table, the elements contain the same number of outer electrons but an extra outer election shell each time.

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

What happens to the state of elements as you move along a period?

A

Going along a period elements move from metallic to non-metallic and add an outer electron each time.

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

What of the first 20 elements in the periodic table are metallic lattices?

A 
Li
Be
Na
Mg
Al
K
Ca
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
6
Q

What are the first 20 elements in the periodic table are covalent molecular

A 
H2
N2
O2
F2
Cl2
P4
S8
Fullerenes (e.g. C60)

‘Some People Never Have Other Fresh Clothes’ + fullerenes

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

What is the first 20 elements in the periodic table are covalent networks

A

B
C (diamond, graphite)
Si

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

What is the first 20 elements in the periodic table are monatomic

A

Noble gases

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

Covalent radius meaning

A

The covalent radius as a measure of the size of an atom.

It is defined as half the distance between the nuclei of two bonded atoms.

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

What happens to the covalent radius across a period?

A

Across a period, the covalent radius decreases because of increased nuclear charge (electrons are attracted closer to the nucleus).

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

What happens to the covalent radius going down a group?

A

Going down a group, the covalent radius increases as the number of occupied electron shells increases

(More shells = bigger atom)

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

First ionisation energy definition

A

The first ionisation energy is the energy required to remove one mole of electrons from one mole of atoms in the gaseous state.

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

Second ionisation energy definition

A

The second ionisation energy is the energy required to remove the second more of electrons in the gaseous state.

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

What happens to the ionisation energy across a period

A

Across a period that ionisation energy increases because of increased nuclear charge. (So more energy is required to remove 1 mole of electron)

(Greater pull on the electrons so more energy required to remove them)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
15
Q

What happens to the ionisation energy going down a group

A

Down a group, ionisation energy decreases because of increased electron shells which means there is an increased shielding affect due to the inner electrons.

(Held less strongly so less energy required to remove the electron)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
16
Q

Electronegativity definition

A

Electronegativity is a measure of an atoms attraction for the shared pair of electrons in a bond.

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

What happens to the electronegativity values across a period

A

Across a period, electronegativity increases because of increased nuclear charge (attracting the electrons more strongly to the nucleus so more energy is required to remove one mole of electron)

(Greater nucleus charge and therefore a smaller covalent radius across a group which allows an atoms nucleus to have a greater force of attraction for electrons.)

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

What happens to electronegativity values down a group

A

Going down a group, electronegativity decreases due to the screening affect. (As a result of shielding and the increased covalent radius the outer electron requires less energy to be removed).

(Inner electrons will shield the nuclear charge)

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

What usually forms a covalent bond

A

A covalent bond usually occurs between non-metal elements.

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

What is a covalent bond

A

A covalent bond is an electrostatic force of attraction between positively charged nuclei and a shared pair of negatively charged outer electrons.

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

When are polar covalent bonds formed

A

Polar covalent bonds are formed when the (different) atoms attractions for the pair of bonding electrons are different.

(They have different electronegativity values)

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

What happens to charges on atoms when polar covalent bonding occurs

A

One atom will become delta positive and the other delta negative.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
23
Q

What atoms becomes Delta negative in polar covalent bonding

A

The atom with the higher electronegativity will be delta negative because it has a stronger attraction for negatively charged electrons

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
24
Q

Are all substances with polar covalent bonds polar molecules?

A

Not all substances with polar covalent bonds will be polar molecules.

If a molecule that has polar bonds has a symmetrical arrangement it will be nonpolar because the overall polarity cancels out

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
25
Polar molecules Vs nonpolar molecules
Polar molecules are molecules that contain polar bonds and are asymmetric. Non-polar molecules may contain polar bonds but they are symmetrical so the overall polarity cancels out.
26
Describe the bonding continuum
The bonding continuum shows the continuum of states from covalent to ionic bonds
27
What is the state of covalent networks at room temperature
Solid
28
What is the state of covalent molecular at room temperature
Gas or liquid
29
What is the state of ionic substances at room temperature
Solid
30
Describe the melting point of covalent molecules
Low melting point
31
Describe the melting point of covalent network
Very High melting points
32
Describe the melting point of ionic bonds
High melting points
33
What is the relationship between solubility and molecular size
Solubility decreases as molecular size increases
34
Are polar covalent Compounds and ionic substances soluble in water
Polar covalent compounds and ionic substances tend to be soluble in water. (Remember ‘like dissolves like’)
35
Do covalent bonds conduct electricity
Covalent bonds do not conduct electricity except for carbon in the form of graphite
36
Do ionic bonds conduct electricity
Ionic bonds can conduct electricity when molten or in solution
37
What are intermolecular forces
Intermolecular forces act between molecules. These are known as van Der waals forces.
38
State intermolecular forces (3)
London dispersion forces Permanent dipole- permanent dipole attractions Hydrogen bonding
39
Where does London dispersion forces exist and what is their strength
London dispersion forces are the weakest form of intermolecular bonding and the exist between all atoms and molecules
40
What causes dispersion forces
Dispersion forces are caused by uneven distribution of electrons
41
What forms London dispersion forces
London dispersion forces are formed by the electrostatic attraction between temporary dipoles and induced dipoles which are caused by the movement of electrons in atoms and molecules.
42
What makes a London dispersion force stronger
London dispersion forces get stronger when there are more electrons in an atom/molecule
43
Why do all molecules and atoms contain London dispersion forces
They all contain London dispersion forces because they all have electrons
44
When are molecules described as polar
Molecules are polar when they have a permanent dipole (one end of molecule is permanently positive, other permanently negative)
45
What are permanent dipole-permanent dipole attractions
Permanent dipole-permanent dipole attractions are the intermolecular force of attraction between oppositely charged ends of the polar molecules.
46
Are permanent dipole permanent dipole interactions stronger than London dispersion forces
Permanent dipole permanent dipole interactions are stronger than London dispersion forces
47
What are permanent dipole permanent dipole attractions in addition to
Parent dipole permanent dipole attractions between molecules are in addition to London dispersion forces.
48
What are hydrogen bonds
Hydrogen bonds are permanent dipole – permanent dipole interactions found between molecules which contain highly polar bonds (They are electrostatic forces of attraction between molecules that contain highly polar bonds) - 3 elements
49
What can hydrogen bonds form between | Elements, 3
They are usually found in molecules where hydrogen is bonded to very electronegative atoms. Hydrogen - FLUORINE Hydrogen- NITROGEN Hydrogen- OXYGEN
50
What are the strongest intermolecular force
Hydrogen bonds are the strongest intermolecular force
51
Compare the strength of hydrogen bonds to permanent dipole permanent dipole attractions and London dispersion forces and covalent bonds
Hydrogen bonds are stronger than permanent dipole permanent dipole attractions and London dispersion forces but weaker than covalent bonds.
52
Describe how intermolecular forces of attraction affect a molecules physical properties
As the strength of the intermolecular force of attraction increases, so does melting and boiling point and viscosity.
53
Why does ammonia on water have high boiling points
Ammonia on water have high boiling points due to hydrogen bonding
54
What usually dissolves polar molecules
Polar solvents will usually dissolve polar molecules ‘Like dissolves like’
55
What usually dissolves nonpolar molecules
‘Like dissolves like’ Nonpolar solvents will usually dissolve nonpolar molecules
56
What type of solvent as water
Water is a polar molecule so it is a polar solvent
57
What do ionic lattices and polar covalent molecular compounds tend to be soluble in?
Ionic lattices and polar covalent molecular compounds tend to be soluble in water and other polar solvents, due to the attraction between the opposite charges.
58
What do ionic lattices and polar covalent molecular compounds tend to be soluble in?
Ionic lattices and polar covalent molecular compounds tend to be Insoluble in nonpolar solvents, as there is no attraction between the ions and the solvent molecules.
59
Reduction & oxidation definition
Reduction is gain of electrons by a reactant (or loss of oxygen). Oxidation is loss of electrons by a reactant (or gain of oxygen). OIL RIG
60
Redox reaction definition
A Redox Reaction is when an oxidation and a reduction reaction takes place at the same time.
61
What is an Oxidising agent
Oxidising agent is a substance that accepts electrons (helps another reactant to be oxidised by being reduced itself).
62
What is a reducing agent
Reducing agent is a substance that donates electrons (helps another reactant to be reduced by being oxidised itself).
63
Recognising oxidising and reducing agents
Elements with low electronegativities can form ions by losing electrons so act as reducing agents (elements with high electronegativities can act as oxidising agents). Strongest reducing agents are in Group 1 of the Periodic Table (strongest oxidising agents are in Group 7).
64
Oxidising agents location on PT and examples
Oxidising agents are at the bottom of the left-hand side column of the electrochemical series: permanganate (MnO4-) dichromate (Cr2O72-) hydrogen peroxide (H2O2)
65
Reducing agents location on PT
Reducing agents are at the top right-hand column of the electrochemical series.
66
Oxidising agent uses
Oxidising agents can be used to kill fungi and bacteria and also as a bleach.
67
Metallic properties
Metallic elements can conduct electricity in any state. This is because they have delocslised electrons (free to move).
68
Metallic bond definition
A metallic bond is the electrostatic force of attraction between positively charged ions and delocalised electrons.

Z. Hchem (4 decks)

Brainscape helps you reach your goals faster, through stronger study habits.
© 2025 Bold Learning Solutions. Terms and Conditions