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Chemistry > Atomic structure > Flashcards

Atomic structure Flashcards

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1
Q

What did Boyle propose

A

Elements can’t be broken down into anything simpler

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2
Q

What is boyles law

A

Volume is inversely proportional to pressure at constant temperature

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3
Q

What was lavoisiers law of conservation of mass

A

Matter is neither created nor destroyed in a chemical reaction, simply rearranged

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4
Q

What did Davy do

A

Discovered new elements Na, K, Ca etc using electrolysis

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5
Q

What was daltons atomic theory

A

Elements are made of tiny particles, all particles of element are identical, compounds are chemical combinations of these particles

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6
Q

What was dobereiners law of triads

A

Groups of 3 elements with similar properties, one intermediate in properties

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7
Q

What was newlands law of octaves

A

Properties repeat every eight element (when arranged in order of mass)
No noble gases as they were not discovered at the time

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8
Q

What did mendeleevs periodic table look like

A

Arranged elements by property space rather than just weight, left gaps, predicted properties of elements to go in gaps e.g. scandium

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9
Q

What did Moseley do

A

Gave us atomic number (no. Of protons in an atom)

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10
Q

Modern table vs mendeleevs

A

Modern Mendeleevs
-No gaps -gaps left for undiscovered elem’s
-Noble gases present -noble gases absent
-Transition elements in -transition elements not in sep block
Separate block -elements in order of atomic mass
-Elements in order of atomic
Number

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11
Q

What did Democritus (Greek) say

A

Atoms are indivisible

4 elements - earth, wind, fire, water

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12
Q

Describe crookes Maltese cross experiment

A

Hot negative electrode (cathode) produced rays that caused a phosphorescent screen to glow in a vacuum tube.
Crookes called these cathode rays.
Rays could be blocked by a metal cross shape and a shadow of the cross is cast on the end of the tube

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13
Q

What was Thompson’s contribution

A

Deflected cathode rays with charged plates so they must be negative!
Called them electrons(coined by stoney)
Magnet also deflect rays
Proposed plum pudding model of atom - negative electrons in a positive dough

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14
Q

What did Millikan do

A

Discovered the mass of the electron using Oil drop experiment, calculated the mass of the electron using the charge/mass ratio

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15
Q

What did Rutherford do

A

Discovered the nucleus using gold foil experiment
[fired alpha particles from radioactive source in block of lead at very thin gold leaf, alpha particles seen as flashes of light on fluorescent screen]
-almost all passed though - so atom mostly empty space and nucleus is very small
-some deflected - so nucleus positive(like charges repel)
-some bounced straight back - so nucleus is very dense (lot of mass)

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16
Q

What did bohr say

A

Electrons orbit nucleus in shells
Gave us Bohr model
[n=shell number]

17
Q

What did Rutherford discover

A

Protons when bombarding nuclei with alpha particles, suspected other particles were needed to hold protons together

18
Q

What Chadwick discover

A

Neutrons by bombarding Be with alpha particles

19
Q

Describe atoms

A

No charge, tiny, 6x10^23 particles

20
Q

Describe molecules

A

Groups of atoms chemically joined

21
Q

Describe ions

A

Atoms that have a charge

22
Q

What is the mass, charge and location of the proton

A

Mass 1
Charge +1
Location nucleus

23
Q

What is the mass, charge and location of the neutron

A

Mass 1
Charge neutral
Location nucleus

24
Q

What is the mass, charge and location of the electron

A

Mass 0
Charge -1
Location orbiting nucleus

25
Q

What is the principle of the mass spectrometer

A

Positive ions can be separated based on relative mass when moving in a magnetic field

26
Q

What are the steps of the mass spectrometer

A 
Vaporisation 
Ionisation 
Acceleration 
Separation
Detection Display

Velma is a sound dude

27
Q

What are the uses of the mass spectrometer

A

Determining the mass and abundance of isotopes

Analysis of (I) gases from a waste dump 
                      (ii) trace organic pollutants in water
28
Q

What is matter

A

Anything that has mass

29
Q

Isotope

A

Atoms of the same element with the same no of protons and differing numbers of neutrons

30
Q

Relative atomic mass

A

Average mass of an element in its ground state relative to 1/12th the mass of a carbon 12 atom

Chemistry (18 decks)

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