Topic 1 Flashcards

1
Q

What are ions?

A

Ions are charged particles that can be single atoms or groups of atoms.

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2
Q

Why do atoms form ions?

A

To gain a full outer shell.

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3
Q

What happens when an atom gains electrons?

A

It forms negative ions (anions)

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4
Q

What happens when an atom loses electrons?

A

It forms positive ions (cations)

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5
Q

What are group 1 and 2 elements and what are their charges?

A

They are metals
Group 1 forms 1+ ions
Group 2 forms 2+ ions

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6
Q

What are group 6 and 7 elements and what are their charges?

A

They are non-metals
Group 6 forms 2- ions
Group 7 forms 1- ions

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7
Q

What do these elements have in common?

A

They form ions most readily

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8
Q

What is an ionic bond?

A

When a metal and a non-metal transfer electrons so the metal loses atoms (cation) and the non-metal gains electrons (anion) to gain a full outer shell. They are strongly attracted to each other by electrostatic forces.

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9
Q

What structures do ionic compounds have?

A

Giant ionic lattice structures with very strong electrostatic forces of attraction between oppositely charged ions.

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10
Q

Why do ionic compounds have high melting and boiling points?

A

Due to the strong attraction between the ions, it takes a large amount of energy to overcome it.

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11
Q

Why don’t solid ionic compounds conduct electricity?

A

The ions are fixed in place and can’t move. However when they melt, the ions are free to move and will carry an electric current.

Some also dissolve in water easily.

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12
Q

What are the advantages and disadvantages of 2D representations of structures?

A

They are simple and good at showing what atoms something contains and how the atoms are connected but don’t show the shape of the substances or the size of the atoms.

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13
Q

What are the advantages and disadvantages of dot and cross diagrams?

A

Useful for showing how compounds and molecules are formed and where the electrons in bonds/ions come from but don’t show size of atoms/ions or arrangement.

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14
Q

What are the advantages and disadvantages of 3D models of ionic solids?

A

Show arrangement of ions but only show outer layer of substance.

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15
Q

What are the advantages and disadvantages of ball and stick models?

A

They’re good helping visualise structures
They’re more realistic than 2D drawings
Though they have big gaps between the atoms but in reality this where the electron clouds interact.
They don’t show correct scales of ions or atoms

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16
Q

What is a covalent bond?

A

A strong bond that forms when a pair of electrons is shared between 2 atoms

17
Q

What are some examples of molecules with atoms joined by covalent bonds?

A
H2
H20
HCL
CH4
CO2
O2
18
Q

What structures do substances containing covalent bonds usually have?

A

Simple molecular structures

19
Q

Why do simple molecular structures have low melting and boiling points?

A

The atoms in the molecules are held together by very strong covalent bonds but the forces off attractive between the MOLECULES are very weak so little energy is needed to break these intermolecular forces.`

20
Q

What state are most molecular substances at room temperature?

A

Liquids and gases

21
Q

What happens as the molecules get bigger?

A

The strength of the intermolecular forces increase, so more energy is needed to break them so the melting and boiling point increase.

22
Q

Why don’t molecular compounds conduct electricity?

A

They don’t contain any free moving ions/electrons

23
Q

What are the 4 properties of most giant covalent structures?

A
  • All the atoms are bonded together by strong covalent bonds
  • They have very high melting and boiling points so lots of energy is needed to break the bonds
  • they generally don’t have charged particles so don’t conduct electricity
  • they aren’t soluble in water
24
Q

Give 4 properties of Diamond

A
  • its made up of a network of carbon atoms that each form 4 covalent bonds
  • The strong covalent bonds take lots of energy to break so diamond has a high melting point
  • the strong covalent bonds hold the atoms in a rigid lattice structure making them really hard
  • they can be used to sharpen/strengthen cutting tools
  • it doesn’t conduct electricity because it has no free electrons/ions
25
Q

What is a metallic bond?

A

The electrons in the outer shell of metal atoms are delocalised which produce all of the properties

There are strong forces of electrostatic attraction between the positive metal ions and the shared negative electrons.

the forces of attraction hold the atoms together in a regular structure and are known as metallic bonding which very strong

26
Q

What is the formula for moles?

A

Moles= mass x Mr

27
Q

What is the formula for concentration?

A

Concentration= mass of solute/ volume of solute