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Chemistry AS > Atoms, Isotopes and Equations > Flashcards

Atoms, Isotopes and Equations Flashcards

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1
Q

What are the three main subatomic particles in an atom?

A

Proton, Neutron and electron

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2
Q

Where is the proton found?

A

In the nucleus

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3
Q

What is the relative charge and mass of a proton?

A

Charge: 1+
Mass: 1

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4
Q

Where is a neutron found?

A

In the nucleus

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5
Q

What is the relative charge and mass of a neutron?

A

Charge: 0
Mass: 1

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6
Q

Where is an electron found?

A

In the energy levels/ shells around the nucleus

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7
Q

What is the relative charge and mass of an electron?

A

Charge: 1-
Mass: 1/1836

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8
Q

What is the definition for Atomic number (z)?

A

The number of protons in the nucleus and identifies an element

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9
Q

What is the definition for Mass number (A)?

A

Number of protons and neutrons in the nucleus

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10
Q

How can you calculate the number of neutrons?

A

N= mass number - atomic number

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11
Q

What is the number of electrons equal to?

A

The number of protons

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12
Q

What is the definition for an Ion?

A

Positively or negatively charged atoms/ group of atoms where the number of electrons is different from the number of protons

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13
Q

When is an ion formed?

A

When an atom gains or looses electrons

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14
Q

What is a cation?

A

A positive ion

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15
Q

What is a anion?

A

A negative ion

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16
Q

What is the definition for an isotope?

A

Atoms of the same element with the same number of protons and electrons, but different numbers of neutrons.

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17
Q

Why do isotopes have the same chemical properties?

A

Chemical reactions involves electrons, so isotopes of an element have the same chemical properties as they have the same number and arrangement of electrons.

18
Q

What is the definition for relative mass?

A

As atoms are so small chemists use relative atomic masses to compare the masses of atoms, elements an compounds

19
Q

What is the standard measurement of relative masses and why is it used?

A

Carbon-12, 12C is used as the standard measurement of relative masses, as 1/12th of 12C is essentially the mass of a proton/ neutron.

20
Q

What is the definition for Relative isotopic mass?

A

Mass of an atom of an isotope relative to 1/12th of the mass of an atom of carbon-12

21
Q

What is the definition for Relative atomic mass, Ar?

A

Weighted mean mass of an atom of an element relative to 1/12th of the mass of an atom of carbon-12

22
Q

What is a mass spectrometer used for?

A

A mass spectrometer can be used to identify isotopes and their abundances, which can then be used to calculate relative atomic mass

23
Q

What are the 5 steps to mass spectrometry?

A
  1. The sample is VAPOURISED, then IONISED to cations.
  2. Ions are ACCELERATED to EQUAL KINETIC ENERGY so the heavier ions move more slowly towards the detector.
  3. Ions create a signal at the detector, the MORE ABUNDANT ions create a BIGGER signal.
  4. Lighter ions meet the detector first
  5. A computer converter turns the ELECTRICAL signals into a MASS SPECTRUM.
24
Q

What is the equation for calculating Relative atomic mass from mass spectrometry?

A

Ar= Sum(Isotopic mass X abundance) / Total Abundance

25
Q

How many decimal places is Relative atomic mass quoted to?

A

1 d.p

26
Q

What is chemical formulae used for?

A

To tell you the ratio of elements present in a compound

27
Q

What are the 7 diatomic elements?

A

H2, N2, 02, F2, CL2, BR2, I2

28
Q

What are the two element exceptions for structure?

A

P4 and S8

29
Q

When is a ionic compound created?

A

METAL+ NONMETAL

30
Q

When is a covalent compound created?

A

NONMETAL + NONMETAL

31
Q

What are binary compounds?

A

Compounds containing only two elements

32
Q

What is the element number up to Group 7?

A 
Group 1 = 1+
Group 2 = 2+
Group 3 = 3+
Group 5 = 3-
Group 6 = 2-
Group 7 = 1-
33
Q

What are polyatomic ions?

A

Groups of atoms covalently bonded together, they have gained or lost electrons, forming negative or positive ions respectively.

34
Q

What are the first four prefix’s for covalent compounds?

A
  1. mono-
  2. di-
  3. tri-
  4. tetra-
35
Q

What is an ionic equation?

A

Show which ions actually react and leave out ions that remain unchanged, in aqueous solutions before and after the reaction.

36
Q

What is the chemical equation for ammonia?

A

NH3

37
Q

What is the chemical equation for methane?

A

CH4

38
Q

What is the chemical equation for water?

A

H2O

39
Q

What is the chemical equation for hydrogen sulphide?

A

H2S

40
Q

What is the chemical equation for propane?

A

C3H8

41
Q

What is the chemical equation for ethane?

A

C2H6

Chemistry AS (16 decks)

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