Brainscape's Knowledge GenomeTM

Browse over 1 million classes created by top students, professors, publishers, and experts.


See full index

Chemistry for the Life Sciences > Bonding > Flashcards

Bonding Flashcards

1
Q

Noble gases are the most…

A

…unreactive of all the elements.

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

Noble gases have little or no tendency to…

A

…form bonds to other atoms.

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

Except He, all noble gases possess a…

A

…ns^2 np^6 configuration

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

Elements that lack the ns^2 np^6 configuration of noble gases tend to…

A

acquire it (i.e. GAIN, LOOSE or SHARE electrons) through chemical reactions, resulting in formation of compounds, where each element has a FULL and stable outer most electron shell

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

Elements of the d and f blocks also lose or share electrons…

A

…Octet Rule does not apply to them.

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

When forming compounds elements lose, gain, or share electrons so their…

A

…configurations become identical to the nearest noble gas in the periodic table

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

What is an ion?

A

atom (or group of atoms) electrically charged (+ve or –ve) as a result of
the loss or gain of an electron

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

Whats a cation?

A

Ions with a positive charge. (loses an electron)

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

Whats an anion?

A

Ion with a negative charge (gains an electron)

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

Atoms can gain or lose…

A

…one, two, or three electrons.

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

Electron loss or gain doesn’t happen in isolation, but are…

A

…parallel processes

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

Ionic bonds are…

A

…electrostatic attractions between cations and anions

(Lewis structures can help visualise the process)

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

An ionic bond is formed only between a…

A

… metal and a non-metal

i.e. group 1 & 2 elements (metals) with group 6 & 7 elements

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

WHat groups on the periodic table are metals?

A

group 1 and group 2

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

WHat groups on the periodic table are non metals?

A

group 6 and group 7

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

the attraction of oppositely charged ions draws them together releasing energy and causing the ions to form a…

A

…solid array or lattice

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

What is lattice energy?

A

a measure of the stabilisation
caused by oppositely charged ions forming a solid lattice.

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

The term “molecule” is not used when…

A

…referring to ionic substances

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

A covalent bond consists of …

A

…a pair of electrons shared between two atoms as the atoms attempt to acquire noble-gas configurations.

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

The covalent bond is the…

A

…predominant chemical bond

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

The sharing of a pair of electrons =

A

single (covalent) bond

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

Atoms can complete octets by…

A

…sharing more than one pair of electrons

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

What is the Valence Shell Electron Pair (VSEPR) Model?

A
  • Based on the idea that electron pairs will repel each other
  • The electron pairs will arrange themselves around the central atom as far apart as possible, to minimise the repulsion between them
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
23
Q

What does VSEPR Model stand for?

A

Valence Shell Electron Pair (VSEPR) Model

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

What is not shown by the Lewis structure?

A

The shape of the molecule is not shown by the Lewis structure

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

What is the electron domain geometry of minimum repulsion for water?

A

tetrahedral

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

In the VSEPR Model, a bond and a nonbonding pair of electrons define …

A

…locations where electrons are
likely to be found and hence are called electron domains

23
Q

Why do electrons repel each other?

A

bcus they are negatively charged bitch

23
Q

Because electrons are negatively charged they…

A

…repel eachother

23
Q

The best arrangement of a given number of electron domains is…

A

…the one that minimises the repulsions between them

23
Q

Whats the MOLECULAR geometry for water?

A

BENT

23
Q

Why is the shape of water so important?

A

life would not be possible if it
were not bent

23
Q

In H20 (water), is the arrangement of atoms (molecular geometry) linear?

A

No!

23
Q

Ionic bonds and nonpolar covalent bonds represent…

A

…two extremes.

23
Q

How many electron domains in water?

A

4

23
Q

If the two atoms that constitute a covalent bond are identical then there is an…

A

…equal sharing of electrons.

23
Q

Covalent bonding involves the…

A

…SHARING of electron pairs.

SHARING IS CARING BITCH

24
Q

The electron pair that makes up the covalent bond is…

A

… equally shared by the two atoms

24
Q

In ionic bonds (such as in NaCl) there is …

A

…no sharing of electrons.

the 3s electron of Na is completely transferred to Cl

24
Q

Ionic bonding involves…

A

…the COMPLETE TRANSFER of electrons.

25
Q

What is an example of a Non polar covalent bond?

A

The chlorine gas molecule
Cl2 is nonpolar covalent.

26
Q

When does a non polar covalent bond occur?

A

When the two atoms that constitute a covalent bond are identical, resulting in an equal sharing of electrons.

27
Q

If the two atoms that constitute a covalent bond are not identical then…

A

…there can be an unequal sharing of electrons

28
Q

When does a polar covalent bond occur?

A

When the two atoms that constitute a covalent bond are not identical, resulting in an unequal sharing of electrons.

29
Q

The charge difference in polar covalent bonds is a result of…

A

…the unequal attractions the atoms have for their shared electron pair and results in a dipole

30
Q

A polar bond results when…

A

…one of the atoms exerts a greater attraction for the bonding electrons than the other

If this difference in relative ability to attract electrons is large enough, an ionic bond is formed

31
Q

What is electronegativity?

A

Electronegativity is the ability of an atom in a molecule to attract electrons to itself

32
Q

Electronegativity increase as you go…

A

…Up the periodic table or from left to right on the periodic table (across the periods)

33
Q

Electronegativity correlates with…

A

…atomic radii

34
Q

What does electronegativity result in?

A

Correlates with atomic radii –> greater nuclear effect (Zeff) –> valence electrons pulled closer to the nucleus.

35
Q

Intermolecular electrostatic
interactions means water is…

A

…liquid at room temperature
(0 – 100 degrees C)

36
Q

VSEPR model is good at…

A

…predicting molecular shapes, but does not explain why bonds exist between atoms.

37
Q

Lewis theory states that …

A

…covalent bonding occurs when atoms share electrons, which concentrates the electron density between the nuclei

38
Q

What are sigma (σ) bonds?

A

Covalent bonds in which the electron density is concentrated symmetrically
about the internuclear axis

39
Q

What are pi (π) bonds?

A

a type of bond which results from sideways overlap of two p orbitals, in which the overlap regions lie above and below the internuclear axis

40
Q

two regions of overlap constitute a single…

A

… pi (π) bond

41
Q

In almost all cases, single bonds are […] and additional bonds are […].

A

In almost all cases, single bonds are s-bonds and additional bonds are p-bonds.

42
Q

Like electron orbitals around an atom…

A

…bonds have different energy levels.

43
Q

s-orbitals have lower energy than…

A

…p-orbitals

44
Q

How / in what order do electron orbitals fill?

A

s-orbitals have lower energy than p-orbitals > electrons fill at the lowest energy
level first:
s orbitals fill before p
covalent bonds follow the same principle (where double/triple bonds are formed):
σ-bonds are lower energy than π-bonds

45
Q

irrespective of atomic orbitals…

A

…sigma bonds form before pi bonds.

46
Q

Carbon is the…

A

…skeleton of biological molecules.

47
Q

Carbon has the ability to form…

A

…polymerise (form long chains)

This is the basis of all biological macromolecules.

48
Q

Bond orbitals confer bond shape –>

A

–> bond shape confers molecule shape

49
Q

Molecule shape is key to…

A

… life – carbohydrates, proteins, lipids, nucleic acid, hormones, vitamins……

Chemistry for the Life Sciences (12 decks)

Brainscape helps you reach your goals faster, through stronger study habits.
© 2024 Bold Learning Solutions. Terms and Conditions