Brainscape's Knowledge GenomeTM


Top Flashcards (Certified)
All Flashcards

Chemistry 20 > Bonding Unit > Flashcards

Bonding Unit Flashcards

0
Q

What are precious metals? Why are they precious?

A

Metals found in their pure form. Because it is rare to find non-ores in nature

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

What are ores?

A

Metals combined with nonmetals in nature

They are solids

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

What state are metals in pure form? What is the exception?

A

Solids.

Hg - Mercury

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

When nonmetals combined what states do they create?

A

Solids liquids or gases

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

What elements are never found in combined form in nature?

A

Noble gases

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

What is the octet rule?

A

The octet rule states that atoms gain, lose, or share electrons in such a way that they create a full outer energy level

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

How many electrons can be held in each energy level?

A

8e-
8e-
2e-
Nucleus

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

Do elements always follow the octet rule?

A

No, the octet rule is just a guideline

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

What are valence electrons?

A

The electrons in the outermost energy level of an atom

They are the only electrons involved in chemical bonding

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

What part of the periodic table is indicative of the number of valence electrons an element has?

A

Group number

Ignoring the 1 in front of groups above 10

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

What does period number indicate of an element?

A

The number of energy levels occupied by electrons

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

What is an electron dot diagram?

A

A model to show the structure and formation of chemical bonds
Consists of the symbol for the element with the dots representing the valence electrons

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

What is a lone pair?

What is a bonding electron?

A

A lone pair is a full orbital and is not involved in bonding ••
Bonding electrons are half full orbital •

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

What is bonding capacity?

A

The maximum number of single covalent bonds that an atom can form (Equals the number of bonding electron)

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

What is Ionic bonding?

A

Ionic bond is the electrostatic attraction between oppositely charged ions

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

How do you draw electron dot diagrams for ionic compounds?

A

Use brackets around each element
The nonmetal will have dots around it
Put the charges of each element
You may have to draw more than one of the metal and/or nonmetal to balance out the charges
The net charge on the compound must be zero

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

What is a covalent bond?

A

When two nonmetals share a pair of electrons

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

Can ions be formed during a covalent bond?

A

No

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

What are electron dot diagram used to show molecular compounds called?

A

Lewis structures

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

What is different between ionic bonds and covalent bonds?

A

Ionic bonds transfer electrons, covalent bonds share electrons to satisfy the octet rule

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

What is a double or triple bond question

A

The sharing of two or three pairs of electrons between two atoms

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

How do you draw Lewis structures?

A

Place the atom with the most bonding electrons in the centre
Arrange all atoms around it as symmetrically as possible
Share electrons to make sure that all atoms have the octet rule satisfied
Remember that hydrogen only needs to electrons to be satisfied

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

What is a structural formula (diagram) ?

A

Another way of drawing molecules

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

How do you draw the structural formula?

A

Figure out the Lewis structure

Replace all shared pairs of electrons with a line and leave off the lone pairs

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
24
Most metals are solid at room temperature, what does this indicate about the forces holding the atoms together?
Since metals are solid at room temperature, this means that there must be strong attractive forces holding the atoms of the pure metal together
25
What kind of bonds do metals not form? | What kind of bonds do metals form?
Covalent or ionic bonds with other metal atoms | Metallic bonding
26
What happens with the valence electrons in metallic bonding?
All the atoms share all of the valence electrons | The valence electrons are delocalized
27
What does delocalized mean?
It means they are free to move from one atom to another
28
What are metallic bonds made up of?
A network of positive metal ions in a sea of electrons
29
What is a metallic bond
The electrostatic force of attraction between the positive metal ions and the negative sea of electrons
30
What is electronegativity?
The relative measure of the ability of an atom to attract electrons in a chemical bond
31
Where is the electronegativity of an element found on the periodic table?
Below the atomic number and above the chemical symbol
32
What does higher electronegativity mean?
Higher electronegativity means greater attraction (affinity)
33
On the periodic table what is the trend with electronegativity?
Electronegativity increases up a group and increases across a period
34
Do noble gases have electronegativity assigned to them? | Why?
No. Because noble gases do not readily react with other substances
35
How does electronegativity and atom size relate?
As you move from left to right across a period, both the electronegativity and atomic number increase, however, size of the atom decreases
36
Why does size decrease across a period?
The size of an atom depends on the radius of energy level containing the valence electrons In any given period, the valence electrons of each atom occupy the same energy level As you move across the period, the atomic number increases and thus the number of protons in the nucleus increases There is a greater amount of attraction between the nucleus and electrons when there are more protons, therefore the atom is smaller
37
Why does electronegativity increase when atomic size across a period decreases?
It depends on two factors •The distance between the charges - The attractive force between opposite charges decreases with the square of the distance between them • The magnitude of the charges - The attractive force is directly proportional to the amount of charge
38
Will an atom that is small and has lots of protons have a very large amount of electrostatic attraction or a very little amount?
Very large amount
39
Why do big atoms have a small amount of electronegativity?
Because although they have lots of protons, they are shielded by the inner levels of electrons therefore have a small amount of attraction (electronegativity) for the electrons of another atom
40
Do metals have low or high electronegativities And do they gain or lose electrons? What about nonmetals?
Metals have low electronegativities and lose electrons | Nonmetals have hyalite you negativities and will gain electrons
41
What is an ionic bond? What is a covalent bond?
Ionic bonds occur between metals and nonmetals | Covalent bonds occur between nonmetal atoms
42
What happens when two nonmetals have different electronegativities and share electrons?
The sharing is no longer equal and the elements with the higher election negativity pulls the electrons closer to itself
43
What happens when two atoms have the same of electronegativity?
The two nuclei of the atoms will attract electrons with exactly the same strength and the electrons are shared equally between the two atoms
44
What happens when the sharing between two nonmetals are no longer equal? (Regarding charges)
One end of the bond will have a slightly negative charge and the other end of the bond will have a slightly positive charge
45
What are polar covalent bonds? What else are they called?
Bonds that have an equal sharing of electrons | They are also called bond dipoles
46
Bond dipole arrows
Yes no
47
What can you use to determine bond character?
The difference in electronegativity between two atoms
48
Give a clear distinction between ionic and covalent bonding
Bonding is considered a continuum and there is no clear distinction between ionic and covalent bonding
49
What is a crystal structure? what kind of compounds have them?
A 3-D array of alternating positive and negative ions. It is also called a crystal lattice. Ionic compounds have crystal structure
50
Why can't you call the attractive forces in the lattice molecules?
The attractive forces in the lattice are the same, each positive ion is attracted to all of the negative ions around it, and vice versa
51
What does Crystal shape depend on?
The way the ions pack together. The relative size of the ions and the charges on the ions
52
Molecular compounds, where do covalent bonds exist?
Between specific pairs of atoms These compounds exist as molecule that have a given number of atoms and therefore are not necessarily written with the lowest whole number ratio
53
What is the valence shell electron pair repulsion theory?
States that molecules adjust their shapes so that valence electrons are as far away from each other as possible
54
Is electron pair repulsion always equal?
No, it is greatest between two lone pairs, less between a lone pair and a bonding pair, and lowest between two bonding pairs
55
What is the shape of molecular compounds determined by? How many types of shapes are there?
Shape is determined around the central atom | Shapes can be classified into five categories
56
What is the linear shape?
The Central atom is bonded to two other atom and has zero lone pairs, or there is only two items in the molecule
57
What is the trigonal planar shape?
The Central atom is bonded to three other atoms and has zero lone pairs
58
What is the tetrahedral shape?
Central atom is bonded to four other atoms and has zero lone
59
What is a pyramidal shape?
Central atom is bonded to three other atoms and has one lone pair
60
What is the bent shape?
Central atom is bonded to two other atoms and has either one or two lone pairs
61
Memorize the shape code
Sure
62
Can a molecule that contains polar covalent bonds the overall nonpolar?
The individual bonds dipoles are vectors that can be added to each other If the bond dipoles are equal in strength and opposite direction, they cancel each other out, resulting in a nonpolar molecule This canceling happens in symmetrical molecules
63
What happens if the bond dipoles do not cancel?
The entire molecule will have a slightly positive and slightly negative end... Called dipoles
64
What are the general rules for polarity of the molecular shapes?
Tetrahedral – non-polar if all atoms attached have the same pull, polar if different Adams attached Trigonal planer - Same as tetrahedral Pyramidal – polar as long as there is a difference in electronegativity between the atoms Bent – polar Linear – polar or nonpolar… Look at the electronegativity difference
65
What are intramolecular forces?
The forces of attraction within ionic molecules | example: ionic or covalent bonding
66
What are intermolecular forces? Are they strong forces or weak forces? What are they responsible for?
The forces of attraction between molecules They are the weakest of all forces They are responsible for state, melting point, boiling point etc.
67
What are three types of intermolecular forces?
1. dipole dipole forces 2. hydrogen bonding 3. London dispersion forces
68
What are dipole dipole forces?
Electrostatic force of attraction between the dipoles of polar molecules Occurs with polar molecules
69
What is hydrogen bonding?
The attraction between a hydrogen on one molecule which is bonded to oxygen fluorine or nitrogen (HNOF)
70
What are London dispersion forces?
The results of electrostatic attraction of induced dipoles | Occurs with all molecules
71
Compare the forces strength from very low to very high
London dispersion and dipole dipole, hydrogen bonding, ionic bonding, covalent bonding, network covalent
72
What is a network covalent?
Very very high force | Diamond (compressed carbon), SiC, SiO2
73
What does the state of a substance depend on?
The strength of the attractive forces between its particles. Solids have the greatest forces of attraction, liquids have the next greatest, and gases have very few if any intermolecular attraction between the particles
74
What do melting and boiling point indicate about the forces?
Melting and boiling points are indicators as to the strength of attraction within or between molecules
75
What happens when metal melt or boil?
When metals melt or boil, metallic bonds must be broken
76
What happens when ionic compounds melt or boil?
When Island compounds melts or boil, ionic bonds must be broken.
77
What happens when molecular compounds melt or boil?
When the lecture compounds melt or boil, only intermolecular forces must be broken. (Covalent bonds do not break)
78
What do delocalized electrons do to the malleability and ductility of metal? What happens to solids that do not have delocalized electrons?
Delocalized electrons cause bonds to be non-directional, which allows a solid to be malleable ductile Solids without delocalized electrons have directional bonds, which causes them to be brittle and hard
79
What is electric current? Why are metals good conductors of electricity? Why can't solid ionic compounds conduct electricity?
The directional flow of electrons or ions Because the delocalized valence electrons are free to move Because they have valence electrons that are held solidly in place
80
Why are most molecular compounds unable to conduct electricity? Do they conduct electricity when they melt or dissolve in water?
Because in most molecular compounds, valence electrons are not free to move through the molecule and therefore they are not able to conduct electricity When molecular compounds melt or dissolve in water, they don't form ions so they don't carry an electric current

Chemistry 20 (5 decks)

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