Brainscape's Knowledge GenomeTM

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


See full index

Inorganic Chemistry > lesson 3-4 > Flashcards

lesson 3-4 Flashcards

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

what are the vertical columns in the periodic table?

A

represents groups. they are numbered from 1-18. they have the same number of valance electrons.

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

why is there similarities in elements in a group?

A

because they have the same number of valance (outer shell) electrons.

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

what are the horizontal rows in the periodic table?

A

represent a period. which are a group of electrons that have the same number of shells.

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

what are the physical properties of metals?

A

luster, good conductors of heat and electricity, high density, high melting point, ductile, and malleable.

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

what are the chemical properties of metal?

A

easily loses electrons, corrode easily.

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

physical properties of non-metals?

A

no luster, poor conductor, brittle, not ductile, not malleable, low density, low melting point.

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

chemical properties of non-metals?

A

gain electrons easily.

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

which group is in S block?

A

group 1 and group 2

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

which group is in p block?

A

group 13-18

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

which group is in d block?

A

group 3 to 12

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

which group is in f block?

A

lanthanides and actinides.

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

what do atomic properties depend on?

A

the strength of attraction between outer shell and nucleus.

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

what affects the attraction between outer shell and nucleus?

A

the positive charge that attracts the outer shell.

the distance between electrons and the nucleus.

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

what is the core charge and how does it behave down the group and across a period?

A

it’s the attraction between outer shell electron feels towards the nucleus.
group -> constant
period -> increases

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

what is the core charge and how does it behave down the group and across a period?

A

it’s the attraction between outer shell electron feels towards the nucleus.
group -> constant
period -> increases

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

how does the radius of the atom behave in period and a group? explain

A

group -> increases.
because of the increase in the number of outer shells.
period-> decreases
because the core charge increases while the number of shells stays the same.

16
Q

the difference in atomic and ionic radius?

A

anions are larger than the original atom, while cations are smaller.

17
Q

what is ionization energy?

A

the energy to detach one from the natural atom in a gaseous state.

18
Q

how does ionization energy change down the group and across the period? explain.

A

group -> decrease
because size increases which means that the attraction between the outer shell and nucleus is lower.
period -> increase
because the core charge increases and the attraction between the outer shell and nucleus are greater.

19
Q

how is ionization energy found?

A

electron impact and photo electron spectroscopy. which eject the electrons.

20
Q

what is an effective nuclear charge?

A

the magnitude of positive charge that an electron experiences.

21
Q

why does shielding occur and what is shielding?

A

it’s electrons partially shielding other electrons from positive charge of the core.
because of the attractions between the negative electrons and positive core and repulsion of electrons from other electrons.

22
Q

how does the effective nuclear change across a period and down a group? explain.

A

period -> increases.
because core electrons don’t change but nuclear charge changes.
group -> doesn’t change.

23
Q

what is electron affinity? and what does it mean if it has a positive electron affinity?

A

the amount of energy released when a neutral atom gains an electron.
means that it has a lower energy that is better than neutral atom.

24
Q

what is electronegativity and what kinds are there?

A

measure of power when in chemical combination to attract an electron to itself.
symmetrical, asymmetrical.

25
Q

what is bond dissociation energy?

A

the energy required to separate bonded atoms.

26
Q

what is bond enthalpy?

A

change in heat when a bond is broken.

27
Q

what is the method that allred and rocher used to measure electronegativity?

A

the electrostatic force exerted by a nuclear charge on valance electrons.

28
Q

how does moving across a period and down a group affect electronegativity?

A

period -> increases

group -> decreases

29
Q

what is a dipole moment?

A

a molecule that has a side with a negative charge core and a side with a positive charge core.

30
Q

how does a dipole molecule behave in a electrical field?

A

the molecule will line up its negative side to the positive pole and its positive side to the negative pole.

31
Q

polar molecules that don’t have a dipole moment?

A

a linear molecule with two identical bonds.
a planar molecule with three identical bonds.
a tetrahedral molecule with four identical bonds.

Inorganic Chemistry (5 decks)

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