Brainscape's Knowledge GenomeTM

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


See full index

Chemistry > Topic 2: Bonding and Structure > Flashcards

Topic 2: Bonding and Structure Flashcards

You may prefer our related Brainscape-certified flashcards:
Periodic Table flashcards Chemistry 101 flashcards AP® Chemistry flashcards Organic Chemistry 101 flashcards
1
Q

When are ions formed?

A

ions are formed when electrons are transferred from one atom to another

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

What is an ion?

A

Charged particle

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

Define electron transfer

A

when an electron lost by one atom is gained by another

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

What is an anion?

A

Negative ion

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

What is a cation?

A

Positive ion

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

What is electrostatic attraction?

A

Holds positive and negative ions together - very strong

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

what is made when oppositely charged ions come together and form and ionic bond?

A

Ionic compound e.g. Sodium Chloride (NaCl)

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

What properties would you expect a specific ionic compound to have?

A
  1. electrical conductivity - when molten or dissolved (ions in a liquid are free to move and carry a charge)
  2. Melting point - High melting points due to giant ionic lattices held together by electrostatic forces.
  3. Solubility - tend to dissolve in water
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
9
Q

**Remember

A

**Even though ionic compounds contain ions they are neutral overall

**when asked to give formula don’t forget charge and formula

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

What is a giant lattice?

A

Regular structure that is ‘giant’ because its made up of the same basic unit repeated.

** Different ionic compound have different shaped structure but they are all still GIANT LATTICES.

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

What is a single covalent bond?

How is a covalent bond formed?

A

A shared pair of electrons

When 2 atoms share electrons so they both have full outer shells

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

When are molecules formed?

A

When 2 atoms (same or different) are joined by a covalent bond - bond is formed by two atoms sharing a pair of electrons.
^^
And there is a strong electrostaticc attraction between nuclei and shared pair of electrons.

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

How is a covalent bond represented?

A

by a single line between two symbols (usually both non metals)

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

When an atom provides both of shared electrons in bonding this is called…

A

Dative Covalent Bonding

**could be lone pairs

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

What is metallic bonding?

A

Positive metal ions are attracted to delocalised negative electrons - they form a giant lattice.

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

How are metals malleable?

A

one layer of metal ions is separated from the next by layer of electrons. this means layers can slide over one another with causing metal to break

17
Q

How are metals conductive?

A

electricity is a flow of charged particles

in a metal electrons are not attached to any on metal ion and are free to move through the lattice

18
Q

How do we know metals have high melting/boiling points?

A

The electrostatic attraction between the positive metal ions and negative electrons make very strong bond.
Bond takes energy to break!

19
Q

What are bonding pairs and lone pairs?

A

bonding pairs - shared electrons

lone pairs - unshared electrons

20
Q

Describe a charge cloud

A

bonding pairs and lone pairs exist as charge clouds

an area where there is a big chance of finding an electron

21
Q

What is non-polar covalent bonding?

A

When electrons are shared equally

22
Q

What is polar covalent bonding?

A

When electrons are shared unequally

23
Q

What is electronegativity?

A

The ability to attract the bonding pair of electrons in a covalent bond

24
Q

How is electronegativity measured?

A

On a Pauling scale

25
Q

What is the general trend in electronegativity of the periodic table?

A

Increase across a period

Decrease down a group

26
Q

Which element is the most electronegative?

A

Fluorine

27
Q

Which is the least electronegative?

A

Caesium

28
Q

When electrons are ‘partially negative’ what does that mean?

A

It means electrons are more often found closer to the partially negative element

29
Q

Why is Cl-Cl non polar covalent bonding?

A

Because it’s the same atoms of an element bonded together so they have the same electronegativity and are equally shared

30
Q

What is a dipole?

A

A difference in charge between the two atoms caused by a shift in electron density in the bond

31
Q

What is a permanent dipole?

A

If charge is distributed in unevenly over a whole molecule

32
Q

What are molecules that have a permanent dipole called?

A

Polar molecules

Chemistry (2 decks)

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