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Chemistry > The Atom + Arrangements of Electrons in the Atom > Flashcards

The Atom + Arrangements of Electrons in the Atom Flashcards

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1
Q

Chemistry

A

Branch of science that deals with the structure and composition of matter and the reactions needed to change it from 1 substance to another

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2
Q

Matter

A

Anything that occupies space and has mass

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3
Q

Mixture

A

2 or more substances MINGLED together but not chemically combined

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4
Q

an Element

A

a substance that cannot be split into simpler substances by chemical means

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5
Q

Compound

A

2 or more elements chemically combined

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6
Q

Atoms

A

smallest particle of an element that can exist on its own

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7
Q

Molecule

A

2 or more atoms chemically combined together

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8
Q

Ions

A

charged atoms

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9
Q

Cations

A

positively charged ions due to loss of electrons from an atom

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10
Q

Anions

A

negetively charged ions due to gain of electrons by an atom

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11
Q

Prove the particular state of matter

A

(diagram of ammonia and hydrochloric acid meet to create a ring of ammonium chloride)

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12
Q

Law of Conservation of Matter/Energy/Mass

A

Matter is neither created nor destroyed during a chemical reaction, it simply changes from 1 form into another

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13
Q

Discharge Tube

A
  • A long glass tube with a metal electrode at each end of the tube
  • and the gas inside at very low pressure (almost vaccum)
  • passing electricity through tube produced invisible rays,
  • moving from the cathode to the anode
  • > cathode rays causing glass to fluoresce
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14
Q

Diffusion

A

spontaneous spreading out of a substance due to the natural movement of its particles

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15
Q

Brownian motion

A

Random, rapid movement of particles

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16
Q

Name 3 sub-atomic particles (subs.)

A

Protons
Neutrons
Electrons

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17
Q

Prove cathode rays travel in straight lines

A

(William Crooke’s diagram of maltese cross casting shadow in discharge tube)

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18
Q

Prove cathode rays posess energy

A

(William Crooke’s diagram of paddle wheel apparatus)

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19
Q

Dalton’s Atomic Theory

A
  • very small particles called atoms
  • atoms are indivisable and indestructable
  • all atoms identical to each other in mass and chemical properties
  • compounds ->2 or more elements combined together in fixed proportions
20
Q

Ancient Greek Philosophers proposed that…

A

-matter composed by ‘indivisable particles’

21
Q

JJ Thompson found…

A

-cathode rays attracted to positive charged plate = negetively charged particles
-RATIO of ELECTRON CHARGE to ELECTRON MASS
e/m ratio
-plum pudding model

22
Q

Electromagnet

A

a magnet that’s formed by passing a current through a wire wrapped tightly round a piece of metal

23
Q

Deflection

A

moved from its original path

24
Q

In 1891, Johnston Stoney…

A

named the electron

25
Q

Robert Milikan…

A

conducted OIL DROP experiment measuring exact charge on electrons -> substituted the charge into e/m ratio and calculated exact mass of electron

26
Q

Rutherford Alpha Particle Scattering Experiment

A

(diagram of alpha particles fired at gold sheet )

27
Q

[Rutherford Alpha Particle Scattering Experiment]
a VERY LARGE NUMBER of alpha particles…

Therefore…

A

𝗥𝗘𝗦𝗨𝗟𝗧: passed straight through gold foil -> UNDEFLECTED

𝗖𝗢𝗡𝗖𝗟𝗨𝗦𝗜𝗢𝗡 𝗮𝗯𝗼𝘂𝘁 𝗔𝗧𝗢𝗠𝗜𝗖 𝗜𝗖 𝗦𝗧𝗥𝗨𝗖𝗧𝗨𝗥𝗘: Atoms are mostly EMPTY SPACE

28
Q

[Rutherford Alpha Particle Scattering Experiment]
MANY alpha particles…

Therefore…

A

𝗥𝗘𝗦𝗨𝗟𝗧: deflected at small angles and a small number were deflected at larger angles
𝗖𝗢𝗡𝗖𝗟𝗨𝗦𝗜𝗢𝗡 𝗮𝗯𝗼𝘂𝘁 𝗔𝗧𝗢𝗠𝗜𝗖 𝗜𝗖 𝗦𝗧𝗥𝗨𝗖𝗧𝗨𝗥𝗘: Repulsion of particles coming close to small dense concentration of positive charge = NUCLEUS

29
Q

[Rutherford Alpha Particle Scattering Experiment]

a VERY SMALL NUMBER of alpha particles…

A

𝗥𝗘𝗦𝗨𝗟𝗧: bounced back along their own path

𝗖𝗢𝗡𝗖𝗟𝗨𝗦𝗜𝗢𝗡 𝗮𝗯𝗼𝘂𝘁 𝗔𝗧𝗢𝗠𝗜𝗖 𝗜𝗖 𝗦𝗧𝗥𝗨𝗖𝗧𝗨𝗥𝗘: alpha particles colliding head on with NUCLEUS

30
Q

orbit

A

energy level

fixed path that an electron occupies

31
Q

Rutherford also…

A
  • Rutherford’s Model of the atom- NUCLEUS + electrons outside
  • > Knocked out positively charged particles = PROTONS
  • predicted nucleus had other particles wth same mass but NO charge
32
Q

James Chadwick found…

A

NEUTRONS and neutrons having same mass as protons

33
Q

Niels Bohr found…

A

Orbits and energy levels for electrons

34
Q

A.M.U.

A

Atomic Mass Unit

35
Q

Atomic Number (Z) of an element

A

no. of protons in the nucleus of an atom of an element

36
Q

Mass Number (A) of an atom

A

the sum of the protons and neutrons in the nucleus

37
Q

Nuclear format of an element

A

Periodic table elements turned upside down

38
Q

Isotopes

A

atoms of the same element with the same Atomic number but different MASS numbers due to different number of neutrons in nucleus of each atom

39
Q

Reletive Atomic Mass (Aᵣ) of an element

A

The average mass of an atom of an element reletive to ¹⁄₁₂ the mass of a Carbon-12 atom

40
Q

Principle of the Mass Spectrometer

A

positively charged ions are deflected to different extents and seperated on the basis of their reletive masses in a magnetic field

41
Q

[Mass Spectrometer]

Vapourisation

A

inlet that contains a heater to vapourise non-gasous samples

42
Q

[Mass Spectrometer]

Ionisation

A

electron gun fires electrons at sample atoms, knocking electrons out of sample atoms forming positively charged ions

43
Q

[Mass Spectrometer]

Acceleration

A

electric field(negetively charged plates) concentrates ions into narrow beam and causes them to move at high speeds

44
Q

[Mass Spectrometer]

Seperation

A

magnetic field seperates ions based on their masses

45
Q

[Mass Spectrometer]

Detection

A

ions strike a detection screen and the abuncance of each is recorded

46
Q

Uses of the Mass Spectrometer:

A
  • To calculate Aᵣ of an element

- to calculate the masses and abundance of isotopes

47
Q

3 states of matter:

A

Solids
Liquids
Gases

Chemistry (7 decks)

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