Elements of Life Flashcards

1
Q

Define mass number

A

The sum of protons and neutrons in an atom

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2
Q

Define atomic number

A

The number of protons in an atom

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3
Q

Define isotopes

A

An element with the same atomic number but a different mass number

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4
Q

Relative atomic mass is …

A

The weighted mass of an atom of an element relative to one-twelfth of the mean mass of an atom of the carbon-12 isotope

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5
Q

Relative molecular mass…

A

The weighted mean mass of a molecule ina compound relative to the one twelfth of the mean mass of the carbon-12 isotope.

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6
Q

Percentage yield formula

A

Experimental mass/ Theoretical mass x 100

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7
Q

Nuclear fusion is…

A

when two lighter nuclei fuse to form a heavier nucleus of a new element releasing a large amount of energy.

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8
Q

What is a titration?

A

A standard solution of a known concentration is reacted with a solution of unknown concentration to determine the property of the solution

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9
Q

Name the visible light region of the EM spectrum in order of decreasing wavelength and increasing frequency and energy.

A

Infrared , Visible , UV

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10
Q

How is emission spectra formed?

A

When particles in the chromosphere absorb energy, the electrons get excited and are promoted from their ground state to a higher energy level. The particles lose this energy and emit radiation which can be detected due to different wavelengths.

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11
Q

Describe what emission spectra looks like?

A

Black backhround, coloured lines

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12
Q

Describe what absorption spectra looks like?

A

Coloured background , black lines

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13
Q

How is absorption spectra formed?

A

Particles absorb some of the emitted radiation, so the light analysed from stars is missing certain frequencies. The absorption lines appear as black as they are missing frequencies of light as they have been absorbed.

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14
Q

Similarites of emission and absorption

A

As frequency increases, lines converge.
Both are line spectra

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15
Q

Differences of emission and absorption

A

Emission is a black background and coloured lines absorption is the opposite

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16
Q

Li+ -
Na+ -
K+ -
Ca 2+ -
Ba 2+ -
Cu 2+ -

A

Red
Yellow
Lilac
Orange-red
Green
Blue green

17
Q

speed of light =

A

wavelength x frequency

18
Q

energy of a photon =

A

Planck constant x frequency

19
Q

What is Bohr’s theory and what points did he make?

A

Explains why H+ only emits a limited number of specific frequencies.

E- in a H+ exists only in a certain definite energy level

A photon of light is emitted or absorbed when electron changes energy level

energy of a photon is equal to the difference btwn the two energy levels

E= Hv so frequency is proportional to energy

20
Q

How many electrons can each sub shell hold

A

S = 2
P = 6
D =10
F =14

21
Q

What is an orbital

A

A region of space with a high probability of finding an electron.

22
Q

How is ionic bonding formed and properties

A

Formed from electrostatic attraction between positive and negative ions.

It occurs between a metal and a non metal. E- transferred to the non -metal.

Can conduct electricity when molten or aqueous because ions can move .

Can form giant ionic lattice like NaCl

23
Q

Cations are…
Anions are…

A

Positive
Negative

24
Q

How are covalent bonds formed and properties

A

Strong electrostatic attraction between a shared pair of electrons and the nuclei of the bonded atoms

Formed between two nonmetals. Share electrons to create a full outer shell

It cannot conduct electricity.

low mp/bp

25
Q

What are dative covalent bonds

A

When both of the electrons in the shared pair are supplied from a single atom

26
Q

Macromolecular covalent structures are….

A

covalently bonded into a giant lattice structure and have a high melting point

27
Q

What is metallic bonding + properties ?

A

A giant lattice of positively charged ions surrounded by a sea of delocalised electrons.

They have very strong electrostatic forces of attractions between the oppositely charged particles.

Malleable as layers of positive ions are able to slide over one another

Good conductors as sea of delocalised electrons are able to move and carry a flow of charge.

High mp/bp

28
Q
A