Busy. Please wait.
or

show password
Forgot Password?

Don't have an account?  Sign up 
or

Username is available taken
show password

why


Make sure to remember your password. If you forget it there is no way for StudyStack to send you a reset link. You would need to create a new account.
We do not share your email address with others. It is only used to allow you to reset your password. For details read our Privacy Policy and Terms of Service.


Already a StudyStack user? Log In

Reset Password
Enter the associated with your account, and we'll email you a link to reset your password.

Remove ads
Don't know
Know
remaining cards
Save
0:01
To flip the current card, click it or press the Spacebar key.  To move the current card to one of the three colored boxes, click on the box.  You may also press the UP ARROW key to move the card to the "Know" box, the DOWN ARROW key to move the card to the "Don't know" box, or the RIGHT ARROW key to move the card to the Remaining box.  You may also click on the card displayed in any of the three boxes to bring that card back to the center.

Pass complete!

"Know" box contains:
Time elapsed:
Retries:
restart all cards




share
Embed Code - If you would like this activity on your web page, copy the script below and paste it into your web page.

  Normal Size     Small Size show me how

GCSE4 Reaction Metal

AQA GCSE Chapter 05 (part 1) reactions of metals

QuestionAnswer
Place the following metals in order of reactivity (most reactive first): Copper, Zinc, Potassium, Gold, Iron, Aluminium Potassium, Aluminium, Zinc, Iron, Copper, Gold. Try this Mnemotechnic: “Pretty Sally Could Marry A Crazy Zulu In Tree Lined House Causing Strangely Glancing People.”
Predict the products when Iron is placed in Copper Sulfate Copper and Iron Sulfate
What would you observe when Iron is placed in Copper Sulfate 1) Identify the products: Copper and Iron Sulfate; 2) Learn colours: Copper Sulfate is blue; Iron Sulfate is very pale green; Copper metal is orange; 3)answer: it would go from a blue solution to a pale green solution
What is the red brown metal formed when Iron is placed in Copper Sulfate 1) Identify the products: Copper and Iron Sulfate; 2) Learn colours: Copper Sulfate is blue; Iron Sulfate is very pale green; Copper metal is orange; 3)answer: teh red-brown metal must be copper (NOT RUST!!!!)
Explain why Iron reacts with Copper Sulfate Because Iron is more reactive than Copper, so iron can “steals” the sulfate from copper
Explain why there is no reaction when you place Copper in Iron Sulfate Because Copper is less reactive than Iron so Copper can NOT steal the sulfate from the iron...
Write the word equation when Iron reacts with copper sulfate Iron + Copper sulfate --> Iron Sulfate + Copper
HIGHER TIER: What is the IONIC equation for the following reaction: Fe + CuSO4 --> Cu + FeSO4 Fe + Cu+2 --> Fe+2 + Cu; the SO4 ion does not appear as it remains the same as a reactant and product
HIGHER TIER: Why is the reaction between Iron and Copper sulfate a redox reaction in terms of electrons? The ionic equation is Fe + Cu+2 --> Fe+2 + Cu; Fe is losing two electrons so Fe is oxidised; Copper is gaining electrons, so Copper is reduced
What is an ore? Rocks that contain enough of a metal compound so that profit can be made when you extract the metal from the metal oxide
"Aluminium + Oxygen --> Aluminium Oxide". What type of reaction is it? Oxidation
Name a metal that can be extracted by heating with Carbon Zinc, Iron or any metal lower than Carbon in teh Reactivity Series
Name a metal that must be extracted by electrolysis Aluminium, Sodium
Name a metal that can be found native Gold , Platinum
Why can Iron be extracted by heating with Carbon? because Iron is LESS reactive THAN Carbon (saying "Iron is not very reactive" is not enough)
Why must Sodium be extracted by electrolysis? because Sodium is MORE reactive THAN Carbon (saying "Sodium is very reactive" is not enough)
"Aluminium + Iron Oxide --> Aluminium Oxide + Iron". What chemical is oxidised? Aluminium
"Aluminium + Iron Oxide --> Aluminium Oxide + Iron". What chemical is reduced? Iron Oxide
What type of compounds are found in metal ores? Mostly Metal Oxides
When you heat Tin Oxide with Carbon, you can extract Tin. Write the word equation. Tin Oxide + Carbon --> Tin + Carbon Dioxide
You get Aluminium when you electrolyse Aluminium Oxide. Write the word equation for the electrolysis of Aluminium Oxide. Aluminium Oxide --> Aluminium + Oxygen
Name the two methods to extract metals from their ores. Heating with Carbon and Electrolysis
Balance the following equation:__ PbO + __ C --> __ Pb + __ CO2 2 PbO + 1 C --> 2 Pb + 1 CO2
Balance the following equation:___ Zn + ___ O2 --> ___ ZnO 2 Zn + 1 O2 --> 2 ZnO
CHALLENGE: Why is Aluminium used for making cans even when Aluminium is so reactive? Aluminium reacts very quickly with Oxygen to form a thin layer of Aluminium Oxide. The Aluminium Oxide is NOT reactive.
Why is Aluminium extracted by electrolysis but Iron extracted by heating with Carbon? Because Aluminium is more reactive THAN CARBON, so the Carbon can not take away the Oxygen; but Iron is less reactive THAN CARBON, so Carbon can take away Aluminium (compare the reativity of metals TO THE REACTIVITY OF CARBON)
Which method would you use to extract Sodium from its ore? Electrolysis (because Sodium is a metal more reactive THAN CARBON) [ALWAYS COMPARE THE REACTIVITY OF THE METAL TO THE REACTIVITY OF CARBON]
Which method would you use to extract Iron from its ore? Heating with Carbon (because iron is less reactive THAN CARBON) [ALWAYS COMPARE THE REACTIVITY OF THE METAL TO THE REACTIVITY OF CARBON]
To make Iron, Iron Oxide is heated with Carbon Monoxide and Carbon Dioxide is formed. Write the word equation for the extraction of Iron. Iron Oxide + Carbon Monoxide --> Iron + Carbon Dioxide
Why must the aluminium oxide be very hot? otherwise the ions can not move
What keeps the electrolyte hot during the process? electrical energy
Why must the process run day and night without stopping? if you stop the process, the aluminium oxide cools down and becomes solid
HIGHER: What happens to the aluminium ions, Al3+, at the negative electrode (cathode)? Write the half-equation (showing electrons) Al+3 + 3 e- --> Al
HIGHER: What happens to the oxide ions, O2–, at the positive electrodes (anodes)? Write the half-equation (showing electrons) 2 O2- --> O2 + 4 e-
Why must the carbon anodes be replaced from time to time? As oxygen is produced, it reacts with the carbon electrode to make Carbon Dioxide: the electrode literally burn!
What is the role of cryolite? to lower the melting point of Aluminium Oxide and thus less energy is needed to melt Aluminium Oxide
HIGHER: What is reduced in 1 Ca + 2 H(+1) --> 1 Ca(+2) + 1 H2 the Hydrogen ion as they are gaining electrons (it goes from a +1 charge to 0 (zero charge)
How do you work out the formula of Calcium Chloride CHARGES: Calcium is +2 ion as it is in group 2; Chloride is -1 ion as it is in group 7; SWAP: Ca1Cl2
How do you work out the formula of Magnesium Nitrate CHARGES: Magnesium is +2 ion as it is in group 2; Nitrate is (NO3)-1 ion LEARN; SWAP: Mg1(NO3)2
How do you work out the formula of Copper(II) Sulfate CHARGES: Copper is +2 ion as indicated by (II); sulfate is (SO4)-2 LEARN; SWAP: Cu2(SO4)2; and cancel both “2s”
State 4 observations when you place an alkali metal in water the fantastic 4"f": Float on water, fizz, flame and gets fmaller
What are the product of reaction between Sodium and water? Sodium Hydroxide and Hydrogen gas
Write the word equation for the reaction of Lithium and water Lithium + Water --> Lithium Hydroxide + Hydrogen; LEARN PATTERN
Write the formula of potassium hydroxide KOH
What is the formula of Hydrogen gas? H2
Write the symbolic equation for the reaction of potassium and Water 2 K + 2 H2O --> 2 KOH + H2; learn the pattern (metal+water--> hydrogen + metal hydroxide); CHECK FORMULAE; this is not an easy equation to balance so maybe learn it altogether?
Which alkali metal is the most reactive? Li, Na or K K
(HIGHER) Balance the half-equation: Al+3 + ____ e- --> Al Al+3 + 3 e- --> Al
(HIGHER) is this half-equation representing an oxidation or a reduction? Explain why. Mg --> Mg+2 + 2e- Mg --> Mg+2 + 2e- is an oxidation because electrons are LOST (OILRIG: Oxidation is Loss and Reduction is Gained)
(HIGHER) is this half-equation representing an oxidation or a reduction? Explain why Al+3 + 3 e- --> Al Al+3 + 3 e- --> Al is a reduction because electrons are GAINED (OILRIG: Oxidation is Loss and Reduction is Gained)
The formula of Sodium Nitrite is Na(NO2). What is the formula of the Nitrite ion? (1=IDENTIFY ION) Sodium is Na; so Nitrite is NO2; (3=work out sign); Na is a metam (+ ion) so Nitrite is a non-metal, a (- ion); (2=UNSWAP) Na is +1 ion (look at Periodic table); so the Nitrite is -1
Explain why metals are malleable because ATOMS are the same SIZE, so when the metal is hit, a LAYER of ATOMS will SLIDE past the other layers (make sure that you use the keywords!)
Explain why alloys are stronger than the pure metals so when the metal is hit, because ATOMS different SIZES, the LAYERS of ATOMS cannot SLIDE past the other layers and the whole structure breaks (make sure that you use the keywords!)
Created by: ursulinechem2