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Chemistry Recap Ppt Flashcards

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1
Q

elements
- helium gas
- gold nugget
- salt
- water

A

the simplest substances in the universe, they are the building blocks of all other substances

e.g.
helium gas = element is helium atoms only

gold nugget = element is gold atoms only

salt = elements are sodium atoms and chlorine atoms

water= element is hydrogen atoms and oxygen atoms

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2
Q

what is made if we dissolved salt in the water?

A

solution

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3
Q

why do pure metals in group 1 and 2 need to be stored in oil?

why don’t group 13 metals need to be stored in oil?

A
  • group 1 and 2 metals are highly reactive with oxygen and water in the air

e.g. sodium and potassium can ignite or explode with water (ms allday experiment)
-> storing them under oil keeps out air and water, preventing dangerous reactions and corrosion.

  • aluminum is less reactive compared to group 1 and 2 metals
  • when exposed to air, aluminium forms a thin layer of aluminium oxide which prevents further reaction
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4
Q

example of group 1 and 2 metals

A
  • sodium
  • potassium
    -calcium
  • magnesium
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5
Q

covalent bonding

A

non-metal atoms held together by sharing electrons forming discrete molecules

covalent bonding = molecules

e.g. In H₂O (water), two hydrogen (H) atoms and one oxygen (O) atom. These atoms are held together by covalent bonds, and the result is a molecule of water.

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6
Q

ionic bonding

A

3D lattice of metal cations and non-metal anions, held together by electrostatic attraction

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7
Q

3 types of bonding

A
  1. metallic bondings (in metals)
  2. covalent bonding (non-metals)
  3. Ionic bonding (metal and a non-metal)
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8
Q

atoms are what?
electrons
cations and anions

A

atoms are neutral since protons are the same as electrons

electrons are negatively charged

cations are positive ions
-> to become a cation, they need to lose electrons

anion are negative ions
-> to become an anion, they need to gain electrons

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9
Q

metal cations are joined by what?

non-metals atoms before ions are joined by what?

A

metal cations joined by metallic bonding

non-metal atoms before becoming ions are joined by covalent bonding

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10
Q

how are metal cations and non-metal anions bonded?

A

metal cations and non-metal anions join together by ionic bonding

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11
Q

example of ionic bonding

A

sodium Na- metal cations join together by metallic bonding

chloride CI2- non-metal atoms joined together by covalent bonding

sodium chloride NaCI - through ionic bonding-> metal cations and non-metal anions are joined together by ionic bonding

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12
Q

ionic/salt compounds meaning + formula

A

metal cations + non-metal anions.

substances made of cations and anions held together by strong electrostatic forces, known as ionic bonds.

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13
Q

4 examples of ionic compounds

A

ionic compounds can be salts

Pyrite (FeS₂)

Rust (Fe₂O₃)

Fluorite (CaF₂)

Halite (NaCl)

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14
Q

compound meaning

A

substance made of 2 more different types of atoms from different elements that are chemically bonded together

example: NaCI is a compound (ionic type of compound)

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15
Q

what are salts made of?

A

salts are made of many anions bonded together into 3D lattices through electrostatic attraction

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16
Q

ionic compound formulas like CaF2 tells you what?

A

tells you the ratio of ions in the lattice
e.g. NaCI
1:1 ratio (6 cations, 6 anions in diagram)

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17
Q

ionic compound naming rules

A
  1. ionic compounds named from cation 1st, anion 2nd
  2. cations have the same name name as their metal element
  3. anions have different names based on the number of oxygen atoms they have

e.g.
cation: ammonium NH4+, hydrogen H+, lithium Li+, potassium K+

anion: hydroxide OH-, chloride CI-, iodide, nitrite, nitrate, oxide

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18
Q

polyatomic ions

A

contains more than one atom bonded together, together they carry a charge
or
group of atoms with charge

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19
Q

anions have different names based on the number of oxygen atoms they have

A

-ide = no oxygen (3-) -> no “O”
eg. nitride N3-, nitride N3- , hydroxide OH-

-ite = some oxygen (2-)
e.g. nitrite NO2-, oxide O2-

-ate = max amount of oxygen (3-)
e.g. nitrate NO3-

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20
Q

describe periodic table metals and non metals

A

right hand side- metal side
left hand side- non-metal side

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21
Q

group 2

A

group 2 (metals cations) loses 2 electrons to form 2+ ions

Mg2+, Be2+, Ca2+

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22
Q

group 13

A

group 13 loses 3 electrons to form 3+ ions

B3+, Al3+

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23
Q

group 14

A

doesn’t lose 4 electrons or gain 4 electrons! they rarely form ions as they prefer covalent bonding which shares electrons instead of gaining or losing

e.g. Carbon forms covalent bonds in molecules like CO₂ by sharing its 4 electrons with oxygen atoms, instead of C⁴⁺ or C⁴⁻ ion.

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24
Q

group 15

A

gains 3 electrons to form 3- ions
N3- = nitride
p3- = phosphide

OR
non-metals can also form 3 covalent bonds (triple covalent bond)

(By sharing 3 electrons instead, they effectively reach 8 electrons in their outer shell just like they would if they gained 3.)

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25
group 16
gains 2 electrons to form 2- ions O2- = oxide S2- = sulfide OR non-metals form 2 covalent bonds (double covalent bond)
26
group 17
gains 1 electron to form 1- ions F1- = fluoride Cl 1- = chloride I1- = iodide non-metal forms one covalent bonds (single covalent bond)
27
group 18
stable noble gases do not form ions
28
groups 3-12
Many transition metals (from group 3 onwards) have more than one possible charge, indicated by Roman numerals. e.g. Iron (III) = Fe3+ Iron (II) = Fe2+ Some transition metals, like silver and zinc, only have one charge, so no Roman numerals are needed in their names. Zinc = Zn2+ Silver = Ag+
29
group 13 and 15
gains 3 electrons to form a negative ion (anion)
30
in single atoms, what are the charges determined from?
in a single atom (monatomics), charge results from having either more electrons or less electrons than protons
31
negative charge (anions) =
more electrons than protons
32
positive charge (cations)
less electrons than protons
33
how is nitrate a polyatomic anion?
(NO₃⁻) consists of more than one atom. one nitrogen (N) atom and three oxygen (O) atoms, and it carries a negative charge (-1). Since it has multiple atoms, it's called polyatomic, and because it has a negative charge, it’s an anion.
34
air is a mixture of gases:
nitrogen gas 78% air oxygen gas 21% air carbon dioxide gas 0.04% air water gas (depends on humidity) also has hydrogen gas
35
what are clouds?
clouds are small droplets or ice crystals floating in the atmosphere
36
how does covalent bonding create molecules?
1. 2 hydrogen atoms 2. non-metal atoms (hydrogen has 1 electron) share valence electrons to complete their outer-shells = covalent bonding 3. new electron pairs are free to move around each nucleus 4. molecules are discrete (individual) groups of non-metal atoms joined together by covalent bonds e.g. hydrogen molecules are a group of atoms like oxygen and hydrogen
37
carbon dioxide molecule glucose molecule
co2 C6H12O6
38
how much electrons to reach a full valence shell?
8 electrons 2,8,8
39
what diagram do we use to represent covalent bonding
lewis dot diagrams and line diagrams
40
state 3 examples of covalent bonding
1. Cl2 2. H2 3. CO2
41
How is carbon a central atom?
Carbon is the only atom that can form single, double and triple covalent bonds. -> so carbon is a central atom in biochemistry
42
How to name covalent compounds
- similar to naming ionic compounds, but now using prefixes to identify how many of each atom in the covalent molecule 1= mono 2= di 3= tri 4= tetra 5= penta 6= hexa 8= octa 10= deca carbon dioxide carbon monoxide
43
how to identify ionic compound
iconic -> metal + non-metal
44
how to identify covalent compound
covalent -> non-metal + metal
45
magnesium chloride: ionic or covalent?
ionic
46
disulphur mononitride: ionic or covalent?
covalent
47
aluminium oxide: ionic or covalent?
ionic
48
tetracarbon dioxide: ionic or covanent?
covalent
49
Law of Conservation of Matter
atoms cannot be created or destroyed, therefore, there are the same number of atoms before and after a chemical reaction instead, you can just rearrange atoms to create new substances
50
molecules meaning
group of two or more atoms that are held together by attractive forces
51
Law of conservation of Mass
mass is neither created nor destroyed in any chemical reaction
52
equations must be what? why?
equation must be balanced because of the principle of the "conservation of matter". -> it must have the same number of atoms of the same kind on both sides
53
label equation structure
reactants and products
54
describe NH3 and NO
if N appears same number on both sides, the coefficient for NH3 same as NO
55
4 types of chemical reactions
1. combination 2. decomposition 3. single displacement 4. double displacement
56
combination reactions
- elements or compounds combine to form one product H2 + 02 -> H20
57
combination general form
A + X -> AX
58
combination reactions 3 examples
1. Magnesium combines with oxygen to form magnesium oxide magnesium + oxygen -> magnesium oxide Mg + 02 -> Mgo (balance) 2. Hydrogen gas and oxygen gas combined to form water hydrogen + oyxgen -> water H2+02 -> H2O 3. metal iron combines with sulphur power to form iron (ii) sulfide iron + sulfur -> iron (ii) sulfide Fe + S -> FeS
59
decomposition reactions
one substance splits to form 2 or more substances
60
combination general form
AX -> A + X
61
decomposition reactions 2 examples
1. Copper carbonate heated -> decomposes into solid copper oxide and carbon dioxide gas copper carbonate -> copper oxide + carbon dioxide CuoCO3 -> Cuo + CO2 2. Liquid water passing electric current decomposes into hydrogen gas and oxygen gas water -> hydrogen + oxygen H2O -> H2 + O2
62
single displacement reactions
an element like metal reacts with a compound and replaces another element from the compound
63
single displacement general form
A + BX -> AX + B
64
single displacement e.g. 1 (zinc)
1. metal displacement reaction (more reactive metal displaces less reactive metal from its compound) when zinc strip is placed in copper sulfate solution, copper solid and solution of zinc sulfate are formed zinc + copper sulfate -> copper + zinc sulfate Zn + CuSO4 -> Cu + ZnSO
65
single displacement e.g. 2 (copper wire)
2. metal displacement reaction when copper wire is placed in dissolved silver nitrate solution, crystals of silver and solution of copper nitrate are formed. copper + silver nitrate -> silver + copper nitrate Cu + AgNO3 -> Ag + Cu (NO3)2
66
single displacement e.g. 3 (hydrogen displacement)
3. hydrogen displacement reaction (reactive metals displace hydrogen from acids) when magnesium metal is placed in HCI hydrochloric acid, hydrogen gas and magnesium chloride solution are made Magnesium + hydrochloric acid -> hydrogen + magnesium chloride Mg + HCI -> H + MgCl3.
67
single displacement e.g. 4 (hydrogen displacement)
4. hydrogen displacement reaction (reactive metals displace hydrogen from acids- hydrogen made from hydrochloric acid!) when zinc metal is placed in the hydrochloric acid (HCI), hydrogen gas and zinc chloride solution are made zinc + hydrochloric acid -> hydrogen + zinc chloride Zn + HCI -> H + ZnCI
68
reactivity series of metals
the arrangement of metals in the descending order of their reactivities up = high reactivity low = unreactive
69
what does the reactivity of metals depend on?
how easily they give up their outer shell electrons
70
Acronym for reactivity series
please stop calling me a careless zebra, instead try learning how copper saves gold MOST REACTIVE Please - potassium Stop - sodium Calling - calcium Me- magnesium A- aluminium Careless- (carbon) Zebra- zinc Instead- Iron Try- tin Learning - lead How- (hydrogen) Copper- copper Saves- silver Gold- gold LEAST REACTIVE
71

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