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Science > Chemistry Mid-Topic Test - Year 10 > Flashcards

Chemistry Mid-Topic Test - Year 10 Flashcards

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1
Q

What is an Atom

A

Smallest part element can be broken down into

Consists of protons, neutrons, electrons

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2
Q

What is the Nucleus

A

Center of the atom, consists of protons and neutrons

High density, small volume

Positively charged

99.9% of mass

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3
Q

What are Isotopes

A

Atoms of same element but contains different number of neutrons in nucleus

Main difference from original element is mass

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4
Q

What is Electron Configuration

A

Way of writing amount of electrons in each shell

  • First shell takes 2 electrons
  • Second shell takes 8 electrons
  • Third shell takes 8 electrons
  • Fourth shell takes 8 electrons (Need to only know up to 2)
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5
Q

What happens across a period in atoms

A

Across a period the size of the atom decreases

  • As electrons are attracted more strongly to nucleus (More protons in nucleus)
  • Chance of gaining electrons and forming negative ions increases
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6
Q

What happens in groups in atoms

A

Same number of valence electrons

  • Group number tells us the charge and how many valence electrons it has

They form the same number of bonds

Atoms get bigger down a group
- They hold their electrons less tightly (Even though they have more protons, there are more shells)

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7
Q

What happens on left hand side of periodic table

A

Forms positive ions

As you go down group, forms ions easier, as the valence electrons are further from nucleus (More shells), so they let go of them easier (Francium is the weakest)

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8
Q

What happens on right hand side of periodic table

A

Forms negative ions

As you go to top of group, forms ions easier, as the valences are closer to nucleus (Less shells), so they can pull in more

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9
Q

What is the Noble Gases Pattern

A

Noble gases unreactive

  • Their outermost shell is always full (8 electrons, except Helium)
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10
Q

What is Electronegativity

A

Ability of an atom to attract additional electrons

As you go from left to right of periodic table, electronegativity increases

  • Means the size of the atom gets smaller, increasing the attraction of electrons
  • This is because the nucleus becomes more positive (Has more protons), pulling electrons in closer

As you go from up to down of periodic table, electronegativity decreases

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11
Q

What is a Compound

A

Substance made up of 2 or more different elements in fixed ratio

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12
Q

What are ionic bonds

A

Metal with nearly empty outher shell reacts with non-metal with nearly full outer shell

Where the metal gives their electron to non-metal, so both get full shells

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13
Q

What is the ionic bonding

A

Each ion in ionic compound is held in place by electrostatic attractive forces

  • Held together as opposite ions attract (Anions & Cations)

Ions form crystal lattice made of ionic bonds

  • Each positive ion surrounded by 6 negative ion, vice versa
  • Keeps formation in place
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14
Q

What are ionic compounds

A

Compounds that consist of ions

Consists of metal and one or more non-metals

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15
Q

Properties of ionic compounds & ionic bonds

A

Conductive
Hard
High melting point & boiling point
Soluble
Brittle
- Force applied = Puts positive ions next to eachother, shattering the compound
– Due to repulsion of like charges
– Example: Salt (NaCl)

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16
Q

Solubility process of ionic compounds

A

For Ionic Solids That are Soluble:

Lattice structure of ionic bonds disrupted by water molecules

After dissolving, individual ions are scattered through solution

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17
Q

Flow of Charge in Ionic Compounds

A

Solids:
Ions in lattice fixed in position
They don’t move = No charge flows

Liquid:
Ions in lattice can move
Charge flows = Conducts electricity
Ions go towards their opposite charge (Positive to negative)

18
Q

What are Covalent Bonds

A

Form when two non-metal atoms with nearly full outer shells share electrons

Neither one gives away an electron

Diagrams mainly shown through electron dot diagrams

They make molecules
- Specific atoms joined by sharing electrons

19
Q

How are Covalent Bonds Formed

A

Non-Metals hold onto valence electrons

  • Can’t give them away electrons to bond
  • Though still need noble gas configuration
  • They get it by sharing valence electrons with each other

– = Both atoms get to count electrons toward noble gas configuration

20
Q

What are the 2 kinds of molecules formed

A

Molecular compounds

Diatomic Molecules

21
Q

How are Molecular Compounds formed from covalent bonds

A

Sharing electrons of different elements

Eg. NaCl, Sodium and Chloride share atoms

Low melting & boiling points

Molecular formula shows type & number of atoms in molecule
- Not ratio, actual amount
- Doesn’t tell you how atoms arranged

22
Q

How are Diatomic Molecules formed from covalent bonds

A

8 elements that always form molecules

  • Elements: Hydrogen, Nitrogen, Oxygen, Fluorine, Chlorine, Bromine, Iodine, Astatine

– All the -ogens, -ines
– Basically, Oxygen by itself means O2

  • Easy way to remember, 1 + 7 pattern on periodic table
23
Q

What are Single Covalent Bonds

A

Sharing of two valence electrons

Only between non-metals, and hydrogen

Difference from ionic bond because they form molecules

  • Two specific atoms joined
  • In ionic solid, you can’t tell which atom electrons moved from/to
24
Q

What are Multiple Covalent Bonds

A

Atoms that share more than one pair of valence electrons

  • Double bond = Atom shares two pairs (4) of electrons
  • Triple bond = Atom shares three pairs (6) of electrons
25
Q

How to figure out if you need multiple Covalent Bonds

A

Add up all current valence electrons

Add up all needed electrons for noble gas configuration

Subtract

Divide by 2

Gives bonds

If bonds > atoms, need multiple bonds

26
Q

How to figure out if you need multiple Covalent Bonds

A

Add up all current valence electrons

Add up all needed electrons for noble gas configuration

Subtract

Divide by 2

Gives bonds

If bonds > atoms, need multiple bonds

27
Q

What are Ions

A

Electrically charged, formed when atoms gain / lose electrons to fill shell

Fills shell to become more stable

Electrons that are gained by negative ions came from an ion
- That ion released an electron and became positive

28
Q

What are Cations

A

If atom loses electrons to fill shell = Positive ion (Cation)
- Forms on left hand side of periodic table

Atoms that have few valence electrons that don’t attract as much

29
Q

What are Anions

A

If atom gains electron = Negative ion (Anion)
- Forms on right hand side

Atoms with many valence electrons gain electrons forming negative ions

30
Q

What are Ionic Substances

A

When an element from the left hand side joins with element from right hand side, the left hand side gives electron to right hand side

31
Q

How do you name Metallic Substances

A

Element name

32
Q

How to name Covalent Molecular Substances

A

Element further left named first, keeps its normal name
- If two elements in same group, element further down named first

Element further right (Higher if in same group), named second
- End of its name changed to end in ‘-ide’
– Eg. Fluoride, Oxide, Sulfide, Bromide

33
Q

What are the Prefixes for naming Covalent Molecular Substances

A

Used to indicate if more than one element present in molecule
- 1 = Mono
- 2 = Di
- 3 = Tri
- 4 = Tetra
- 5 = Penta

If first element has one atom, prefix mono not used

Molecules composed of one element only, get name of original element

34
Q

How to name Ionic Compounds

A

Metal / Positive Ion named first
- Keeps normal name

Non-Metal / Negative Ion named second
- End of its name changed to end in ‘ide’
– Eg. Fluoride, Oxide, Sulfide, Bromide

35
Q

How to write formulas for Metallic Elements

A

Single symbol that does not indicate number of atoms present
- Eg. Na, Al, Fe

36
Q

How to write formulas for Ionic Compounds

A

Positive ion (Usually metal ion) written first

Negative ion (Usually non-metal ion) written second

Number of each ion adjusted so that positive charge = Negative charge

  • Subscripts used to indicate number of ions present

–Shows ratio, not actual amount

  • Use ‘drop and swap’ method
37
Q

How to write formulas for Covalent Substances

A

Element further left named first
- If two elements in same group, element further down named first

Element further right (Higher if in same group), named second

Number of each ion adjusted so that charges are equal

  • Subscripts used to indicate number of ions present
  • Use ‘drop and swap’ method
38
Q

Dissolving Substances Rule

A

Attractive forces between substance dissolving (Solute) & water (solvent), are stronger than attractive forces between solutes alone

  • If happens = Solute dissolves
39
Q

What are Solutions

A

Form when particles of solute (Particles) enter the solvent (Water)

Have uniform properties

May be coloured, but always clear

40
Q

What happens when you put a battery into water

A

If you put battery into water

  • All positive ions go to negative electrode (Negative battery side)
  • All negative ions go to positive electrode (Positive battery side)
41
Q

What is a precipitation reaction

A

Insoluble solid that can form as part of reaction between two ionic solutions

Solubility of compound can be predicted from solubility rules

42
Q

What is Solubility

A

Ability for a solute to dissolve in a solvent to make a solution

Can use solubility table to check if compounds form solutions or precipitates

Science (5 decks)

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