Chemistry Flashcards
(77 cards)
1
Q
What charge does a neutron have?
A
Neutral
2
Q
What charge does an electron have?
A
Negative
3
Q
Electron configuration
A
2,8,8
4
Q
Atomic mass=
A
protons + neutrons
5
Q
First 20 elements
A
Hydrogen Helium Lithium Beryllium Boron Carbon Nitrogen Oxygen Fluorine Neon Sodium Magnesium Aluminium Silicon Phosphorus Sulphur Chlorine Argon Potassium Calcium
6
Q
Chemical elements for hydrogen
A
H
7
Q
Chemical element for helium
A
He
8
Q
Chemical element for lithium
A
Li
9
Q
Chemical element for beryllium
A
Be
10
Q
Chemical element for boron
A
B
11
Q
Chemical element for carbon
A
C
12
Q
Chemical element for nitrogen
A
N
13
Q
Chemical element for oxygen
A
O
14
Q
Chemical element for fluorine
A
F
15
Q
Chemical element for neon
A
N
16
Q
Chemical element for sodium
A
Na
17
Q
Chemical element for magnesium
A
Mg
18
Q
Chemical element for aluminium
A
Al
19
Q
Chemical element for silicon
A
Si
20
Q
Chemical element for phosphorus
A
P
21
Q
Chemical element for Sulfur
A
S
22
Q
Chemical element for Chlorine
A
Cl
23
Q
Chemical element for Argon
A
Ar
24
Q
Chemical element for potassium
A
K
25
Chemical element for calcium
Ca
26
What charge does a proton have?
Positive
27
Electric Charge for a nucleus
Positive
28
Electric Charge for an atom
Neutral
29
Formula for Electrons
2n squared
30
Put protons, atoms, electrons and neutrons in order of lightest to heaviest
Electrons, Protons, Neutrons, Atoms
31
How many elements are there?
118
32
Ion
Is an atom that has gained or lost its valance electrons.
33
When atoms gain an electron what charge do they obtain?
Negative Charge
34
What charge do atoms obtain when they loose an electron?
Positive
35
What is the name for a positively charged electron?
Cation
36
What is the name for a negatively charged atom?
Anion
37
What is an isotope?
An atom with the same number of protons but differing number of neutrons than per usual this altering the atomic mass.
38
What is another word for electron shells?
Energy Levels
39
Element Defintion
A substance composed of atoms with the same atomic number. The most pure form of substance.
40
Ground State-Defintion
Lowest energy arrangement of an atoms electrons in energy shells.
41
What direction do the groups on the periodic table go?
Vertically
42
What direction do the periods on a periodic table go?
Horizontal
43
How can it be figured out which group an element is in?
The number of electrons in the valance shell
44
How can it be figured out with period the element is in?
How many electron shells that the element has.
45
Define covalent bonding.
The sharing of electrons between non-metallic elements. They bond with each other to form a new substance and fill each other outer shell so that the shell is satisfied.
46
What two types of elements is covalent bonding between?
Non-metallic elements
47
What two types of elements is ionic bonding between?
Metal and Non-Metal elements
48
Valance Shell Defintion
The last electron shell of an element, this shell will contain the highest energy level.
49
How can electrons jump for shell to shell?
If electrons are provided with more energy they move away from the nucleus further out and they jump from inner shells to outer shells.
50
How many valance electrons do the Nobel gases have?
None they are satisfied elements.
51
What causes a positively charged atom to be like this?
More protons then electrons.
52
What causes a negatively charged atom to be like this?
More electrons than protons
53
Which type of elements are most likely to loose electrons?
Metallic
54
Which type of elements are most likely to gain electrons?
Non-Metallic
55
Explain and Define Ionic Bonding
Metallic elements loosing and electron and transferring them to a non-metallic element so that each element has a full set.
56
Which type of element is the most reactive?
Metallic
57
Which type of elements does metallic bonding occur between?
Metal and Metals
58
Fill in the blanks
| Metal atoms ________ electrons to form ________ ions which have more ________ than _______.
Loose
Positive
protons
Electrons
59
Fill in the blanks
| Non-metal atoms _________ electrons to form __________ ions which have more ________ than protons
Gain
Negative
Electrons
Protons
60
Why are metals such good conductors of electricity?
They have a weak structure so electrons can be free moving. a the see of free electrons allow metals to carry electrical currents.
61
Whittier are electrons attracted to?
As electrons are negatively charged they are attracted to the positive protons, in the nucleus. This keeps the electrons in orbit.
62
Which shell is most attracted to the nucleus?
The first one, as its closest which makes it the lowest energy
63
When do electrons have the highest energy?
When they are in the outer shell. They have less of an attraction to the nucleus.
64
What is a firework?
The explosion energy causes the electrons to jump shells. As they return to the 'ground state' energy gets released as light
65
What is a chemical formula?
| What does this chemical formula tell you H20?
A formula that tells you what elements make up the substance and in what proportions.
In H2O
There are 2 hydrogens bonded to an oxygen.
66
What's bigger? Protons or Neutrons
Neutrons slightly
67
Monatomic
Atoms that exist on their own, without bonding with others.
68
What is a lattice and how is it formed?
A lattice is formed when electrostatic forces are pulled together to form a strong ionic bond. Each ion is surrounded by an opposite charge that it is being attracted to building up a three dimensional structure known as a lattice.
69
What type of force pull negative and positive ions together?
Electrostatic
70
What number group is the Nobel gases and what is so special about them?
They are number 18 and then are monatomic atoms, known for their intense stability.
71
Do metal atoms have a strong or weak bond in regards to their electrons?
Weak
72
Do non- metal atoms have a strong or weak bond in regards to their electrons?
Strong
73
What group would an atom be that had an electron configuration of 2,8,7?
7
74
What period would an atom that had an electron configuration of 2,8,18,8,2 be situated in?
5
75
Name two forms of carbon that are lattice structures?
Diamond and Graphite
76
Explain why Nobel gases tend not to form bonds?
Because they are stable and are satisfied as the occupy full outer electron shells.
77
If an atom has an electron configuration of 2,6 (oxygen) how many covalent bonds will it need to be satisfied?
2
