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Chemistry > Module 3 - periodic table and energy > Flashcards

Module 3 - periodic table and energy Flashcards

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1
Q

How are elements aranged in the periodic table?

A

proton number

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2
Q

What are the names of groups 1 2 7 and 8?
What is the name of the elements in the middle of the periodic table?

A

Alkali metals Alkaline earth metals Halogens Noble Gasses
Transition metals

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3
Q

Which elements exist as diatomic molecules?

A

H2 N2 O2 Halogens: F2 Cl2 Br2 I2
Have No Fear Of Ice Cold Beer

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4
Q

Why do noble gasses have the lowest melting point?

A

Exist as single atoms

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5
Q

Define metallic bonding

A

Electrostatic attraction between metal cations and delocalised electrons from the outer shell

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6
Q

Why do melting points increase across the period?

A

More delocalised electrons
Charges of cations increase
smaller ion = higher charge density:ratio of charge to volume

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7
Q

Define giant covalent structure and their properties

A

Network of covalently bonded atoms
High melting points

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8
Q

Define allotrope

A

pure forms of the same element that differ in structure

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9
Q

Group 2 reacts with water to produce …

A

hydroxides and hydrogen gas

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10
Q

Group 2 reacts with diluted acids to produce …

A

salts and hydrogen

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11
Q

They burn in oxygen with what characteristic colour?

A

Brick red

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12
Q

What is the test for Ba 2+ ions?

A

White pricipitate forms

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13
Q

What are the periodic trends of alkaline earth metals?

A

Atomic and ionic radius increases down group - more shells
Ionisation energy decreases down group
Reactivity increases down group
Melting points decrease down group
Solubility of oxides and hydroxides increase down group

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14
Q

What is the trend in the halogen group?

A

Less electronegative down group
Less reactive down group
Melting point/boiling point increase down group
Larger molecules
more electrons
stronger london forces

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15
Q

What are some disadvantages of water treatement with chlorine?

A

Cl2 harmful and toxic - irritates respiritory system:liquid chlorine burns eyes/skin
Cl2 reacts with organic compounds to form chlorinated hydrocarbons- carcinogenic

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16
Q

What are some alternitives to treating water with chlorine?

A

ozone
Uv light

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17
Q

What are the tests for all the halides

A

F- no precipate doesn’t dissolve
Cl- White precipitate dissolves in diluted NH3
Br- crem precipitate dissolves in concentated NH3
I- yellow precipitate insoluble

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18
Q

How to identify halide ions in displacement reactions

A

F2 yellow gas
Cl2 green gas water-colourless hexane-pale green
Br2 red brown liquid water-yellow/orange hexane-orange/red
I2 black purple solid water-brown hexane-pink/purple

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19
Q

What is the test for carbonates?

A

Fizzing carbonate dissapears

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20
Q

What is the test for CO2?

A

lime water turns cloudy

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21
Q

What is the test for sulphate?

A

white precipitate

22
Q

What is the test for ammonium?

A

litmus paper turns from red to blue

23
Q

What are some common insoluble salts?

A

silver halides
barium sulfate
most carbonates - except sodium potassium and ammonium carbonates
metal oxides

24
Q

What are some common soluble salts?

A

most hydrogen carbonates
most sodium salts

25
Q

what are the standard conditions for enthalpy change?

A

100 kPa 298 K

26
Q

Define standard enthalpy change of reaction

A

the enthalpy change when the reaction occurs in the molar quantities shown in the chemical equation under standard conditions in their standard states

27
Q

Define enthalpy change of formation

A

enthalpy change when 1 mol of a compound is formed from its elements in their standard states under standard conditions

28
Q

Define enthalpy change of combustion

A

the enthalpy change when 1 mole of a substance is completely burned in oxygen under standard conditions, all reactions and products being in their standard states

29
Q

Define enthalpy change of neutralisation

A

the enthalpy change when 1 mole of water is formed from the neutralisation of hydrogen ions by hydroxide ions under standard conditions

30
Q

What is the equation for bond enthalpy?

A

sum of bonds broken - sum of bonds formed

31
Q

Define bond dissociation enthalpy

A

bond dissosiation enthalpy per mole of gaseous compound

32
Q

Define average bond enthalpy

A

energy needed to break one mole of bonds in the gas phase averaged over many different compounds
This value is ALWAYS positive

33
Q

Bond forming … energy
Bond breaking … energy

A

Releases
Requires

34
Q

Define activation energy

A

Minimum amound of energy needed to begin breaking reactant bonds and start a chemical reaction
ALWAYS POSITIVE

35
Q

Which way do arrows point in exo and endothermic reactions?

A

Exothermic down
Endothermic up

36
Q

What is the equation for enthalpy change?

A

q=mcdeltaT
q=enthalpy change m=mass of water c=4.18 deltaT=change in temp

37
Q

What are some reasons for underestimation of enthalpy change?

A

Heat absorbed by container and lost to surroundings
Incomplete combustion
Non standard conditions

38
Q

Define Hess law

A

The total enthalpy change for a reaction is independant of the route taken (as long as initial and final conditions are the same)

39
Q

What are some factors that impact the rate of a reaction?

A

temperature
surface area
catalyst
concentration of reactants
pressure of gasses

40
Q

What are some methods of measuring rate of reaction

A

precipitation
change in mass
volume of gas
titration

41
Q

what is the equation for rate of reaction?

A

difference in concentration/difference in time

42
Q

How do you calculate the gradient of a linear graph?

A

change in Y/change in X

43
Q

Define catalyst

A

Increases rate of reaction by lowering activation energy and providing an alternative reaction pathway. Catalysts are not used up during the reaction (unchanged)

44
Q

What is a homogenous catalyst?

A

same physical state of reactants, forms intermediates

45
Q

what is a hetrogenous catalyst?

A

different physical state to reactant

46
Q

What is a dynamic equalibrium?

A

rates of the foreward and reverse reactions are equal
concentrations of reactants and products remain constant
only in closed systems

47
Q

Define Le Chetalliers principle

A

When the conditions of a system at equalibrium change, the position of the equalibrium shifts in the direction that opposes the change

48
Q

How is equalibrium affected by an increase in pressure?

A

Shifts to the side with fewer moles

49
Q

What is the equalibrium equation?

A

aA + bB - cC + dD double arrows

50
Q

What is equalibrium law?

A

Kc= (C)c (D)d
(A)a (B)b Brackets concentration

51
Q

What is Kc dependant on?

A

Temperature

Chemistry (11 decks)

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