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chemistry > atomic structure, isotopes and formulae > Flashcards

atomic structure, isotopes and formulae Flashcards

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1
Q

What was stated in Dalton’s atomic theory?

A
  • Atoms are tiny particles made of elements
  • Atoms cannot be divided
  • All the atoms in an element are the same
  • Atoms of one element are different to those of other elements
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2
Q

What is the relative mass of a proton

A

1

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3
Q

Define molecular ions

A

Covalently bonded atoms that lose or gain electrons

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4
Q

How do you calculate the number of neutrons?

A

mass number - atomic number

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5
Q

What is the charge of the ion when electrons are gained?

A

Negative

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6
Q

Define relative isotopic mass

A

The mass of an atom of an isotope compared with 1/12th of the mass of an atom of carbon-12

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7
Q

Explain how to calculate the empirical formula

A
  1. Divide amount of each element by mr
  2. Divide answers by smallest obtained value
  3. If it is a decimal divide by suitable number to get a whole number
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8
Q

Which letter represents the mass number?

A

A

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9
Q

Explain the current model of the atom

A
  • Protons and neutrons are found in the nucleus
  • Electrons orbit in shells
  • Most the atom is empty space between the nucleus and the electrons
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10
Q

What were Rutherfords proposals after the gold leaf experiment?

A
  • Most of the mass and positive charge of the atom are in the nucleus
  • Electrons orbit the nucleus
  • Most of atom’s volume is space between the nucleus and the electrons
  • Overall positive and negative charges must balance
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11
Q

How is the mass number calculated?

A

number of protons + number of neutrons

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12
Q

Why do different isotopes of the same element react in the same way?

A
  • Neutrons have no impact on the chemical reactivity

- Reactions involve electrons, isotopes have the same number of electrons in the same arrangement

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13
Q

What are the 4 elements that don’t form ions and why?

A
  • The elements: beryllium, boron, carbon and silicon

- Require a lot off energy to transfer outer shell electrons

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14
Q

What letter represents the atomic number of an atom?

A

Z

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15
Q

The relative isotopic mass is the same as which number?

A

Mass number

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16
Q

What does the atomic number tell us about an element?

A

The number of protons in an atom

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17
Q

What is the charge of a proton?

A

1+

18
Q

What is the relative mass of an electron

A

1/2000

19
Q

How is the periodic group number related to the number of electrons?

A

Represents the number of electrons in an atoms outer shell

20
Q

Define ions

A

Charged particles that are formed when an atom loses or gains electrons

21
Q

How to calculate the relative molecular mass and the relative formula mass?

A

Add up the relative atomic masses of each of the atom making up the molecule/formula

22
Q

Define relative atomic mass

A

The weighted mean mass of an atom of an element compared with 1/12th of the mass of 1 atom of carbon-12

23
Q

What did Thompson discover about electrons?

A
  • They have a negative charge
  • They can be deflected by magnets and electric fields
  • They have a small mass
24
Q

What is the relative mass of a neutron

A

1

25
Q

Define an empirical formula

A

Simplest whole number ratio of atoms of each element present in a compound

26
Q

What is the charge of an electron?

A

-1

27
Q

Explain the plum pudding model

A

Atoms are made up of negative electrons moving around in a sea of positive charge

28
Q

Define an isotope

A

Atoms of the same element with different number of neutrons and masses

29
Q

Which two particles make up most of the atom’s mass?

A

Protons and neutrons

30
Q

How does a mass spectrometer work?

A
  • The ions are vaporised
  • The atoms are ionised by bombarding it with electrons to knock off its own electrons to create a positive ion which create a narrow beam
  • The ions are accelerated via a negatively charged accelerating plate so they have the same kinetic energy
  • Ions are deflected by the magnetic field by their mass/charge ratio
  • The beam of ions passing through the machine is detected electrically, a signal is amplified
    and recorded
31
Q

What two assumptions are made when calculating mass number?

A
  1. Contribution of the electron is neglected

2. Mass of proton and neutron is taken as 1.0 u

32
Q

Do metals gain or lose electrons?

A

Lose electrons to form positive ions

33
Q

What are the uses of mass spectrometry?

A
  1. Identifying unknown compounds
  2. Finding relative abundance of each isotope in an element
  3. Determining structural information
34
Q

What is the location of electrons in an atom

A

The orbitals

35
Q

What particle has the same mass as a proton?

A

A neutron

36
Q

The formula of an ammonium ion

A

NH4+

37
Q

The formula of a sulfate ion

A

SO4 2-

38
Q

The formula of a zinc ion

A

Zn2+

39
Q

The formula of a silver ion

A

Ag+

40
Q

The formula of a carbonate ion

A

CO3 2-

41
Q

The formula of a nitrate ion

A

NO3 -

42
Q

The formula of a hydroxide ion

A

OH-

chemistry (37 decks)

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