Brainscape's Knowledge GenomeTM

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


See full index

Chemistry > Periodic Table > Flashcards

Periodic Table Flashcards

1
Q

What is a molecule

A

Two or more atoms bond by sharing electrons

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

Compound

A

When atoms are from different elements

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

Mass number

A

Number of protons-number of neutrons

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

Neutrons

A

Mass number-atomic number

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

Isotopes

A

Atoms of the same element can have different mass numbers. They have same atomic number but different number of Nuclei

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

Maximum number of electrons for each shell

A

Shell1:2
Shell2:8
Shell3:18
Shell4:32

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

Valence electrons

A

Electrons in the outermost shell of an atom

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

Core charge formula

A

Number protons - inner shell electrons

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

Atomic radius definition

A

Distance from Centre on atoms to valence electrons

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

Electronegativity trends

A

High for non metals
Group 18 no electronegativity
Less pull when valence electrons further from nucleus

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

First Ionisation energy

A

The energy required to remove first valence electron from atom

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

First Ionisation Trends

A

Decreases going down a group
Increases across a period

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

Metallic character

A

Easily lose electrons, conducts electricity and shiny

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

Non- metallic character

A

Non- metals, gain electrons

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

Metalloids

A

Mix of both metallic and non metallic

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

Metallic trend

A

Going across a period decreasing metallic character

17
Q

What is reactivity

A

How easy it is for an atom to gain or lose electrons

18
Q

Reactivity trends

A

Group 1 most reactive followed by group 2 in the metals but in the non metals it’s group 17 followed by group 16
Group 18 no reactivity
Increase as you go up a group

19
Q

Atomic radii trends

A

Decrease from left to right across a period to group 18
Increase as you go down a group

20
Q

Electro negativity trends

A

Group 18 no electronegativity
Increase across a period and up a group

21
Q

why a neutral atom cannot have the atomic configuration of 6 protons, 13 neutrons and 13 electrons.

A

Neutral atoms must have the same number of protons (positively charged) and electrons (negatively charged). If a species had 6 protons and 13 electrons, it would have an overall charge of +7, which would make it a charged species (ion).

22
Q

Tellurium is element 52 and iodine is element 53. Explain why iodine atoms have less mass than tellurium atoms.

A

Tellurium atoms have more neutrons than iodine, resulting in a higher mass number and higher mass.

23
Q

what is an ion?

A

An atom or a molecule that has a positive or negative electrical charge. not neutral charge. (due to the loss or gain of one or more electrons.)

24
Q

Which of the following determines the chemical properties of an element?

A

The chemical properties of an element are determined by the electron configuration of its orbiting electrons as these interact with other atoms to form chemical bonds.

25
Q

How can the periodic table of the elements be used?

A

To predict how atoms of different elements will combine

26
Q

what is an atomic emission spectrum

A

the pattern of lines formed when light passes through a prism to separate it into the different frequencies of light it contains.

27
Q

Emission Spectrum definition

A

Light contains energy. If an atom has extra energy, it can get rid of it by sending out a little packet of light, called a photon. It also works the other way around: if a photon comes near an atom that could use some extra energy, the photon can be absorbed by the atom

28
Q

how many electrons can occupy subshells 1s 2s 2p 3s 3p 3d 4s 4p 4d 4f

A

1s=2
2s=2
2p=6
3s=2
3p=6
3d=10
4s=2
4p=6
4d=10
4f=14

29
Q

Energy consumption of absorption spectra and emission

A

An absorption spectrum
is produced when
atoms absorb energy.

An emission spectrum
is produced
atoms release energy.

30
Q

Appearance of both spectras

A

Absorption spectra show dark lines or
gaps

Emission spectra show colored lines.

31
Q

Energy of an atom both spectrums

A

An atom obtains a higher energy level when an absorption spectrum is
given by that atom.

An emission spectrum is given when an excited atom obtains a lower
energy level.

Chemistry (12 decks)

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