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Chemistry (shubh) > Module 3 > Flashcards

Module 3 Flashcards

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1
Q

How are elements in periodic table arranged

A

By increasing atom/proton number

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2
Q

What is periodicity

A

Repeating trends in physical and chemical properties

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3
Q

Why do elements of dame group have similar chemical properties

A

Same number of electrons in outer shell/same electron config

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4
Q

What is first ionisation energy

A

The energy required to remove 1 mole of electrons from 1 mole of gaseous atoms to form 1 mole of gaseous 1+ ions

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5
Q

Equation for sodiums first ionisation energy

A

Na (g) —> Na+ (g) + e-

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6
Q

Finish sentence
Ionisation energy is affected by how strongly……. are attracted to ….
Stronger the attraction …. energy required to remove electron so ionisation energy is ….

A

Electrons
Nucleus
More
High

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7
Q

3 factors affecting attraction between nucleus and electrons

Brief explain why

A

Nuclear charge: more protons means stronger pull

Atomic radius: distance between outer shell electron and nucleus affects level of attraction

Electron shielding: nucleus and electron attraction partially blocked by inner shell electrons

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8
Q

Why are there large increases in ionisation energy as you jump to different shell
(In same element subsequent further IE)

A

Big reduction in atomic radius and shielding

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9
Q

Why does first ionisation energy decrease down the group

A

Increase in nuclear charge is more than cancelled out by increase in atomic radii and shielding which decreases nuclear attraction between nucleus and outer shell electrons so less energy required to remove electron

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10
Q

General trend in 1st ionisation energy across a period

A

Nuclear charge increases which causes atomic radius to decrease as stronger pull and nuclear attraction between nucleus and outer shell electron increased and require more energy to remove electron
Shielding is same as same shell across period

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11
Q

Explain slight decrease in 1st ionisation energy across period (between some elements)

A

Ionisation that results in full or half full sets of orbitals require slightly less energy

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12
Q

Explain metallic bonding

A

Giant lattice structure of close packed metal cations in a sea of delocalised electrons with electrostatic forces

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13
Q

Why are metals insoluble in water

Why do metals conduct electricity in both states

A

More likely to simply react rather than break apart by solvents

Delocalised electrons act as mobile charge carriers

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14
Q

Explain giant covalent structure

A

Giant lattice of atoms held by covalent bonds which are strong electrostatic attraction between nuclei and shared/bonded electrons

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15
Q

Why are giant covalent structures insoluble in water

Conduct electricity??

Why does it have high mp/bp

A

Bonds too strong to pull apart

Electrons localised and no charged particles so cant carry charge

Strong bonds require more energy to break

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16
Q

Explain simple molecular structures

A

Small groups of covalent bonded atoms with weak intermolecular forces so easy to melt

17
Q

What are the giant covalent elements in period 2 and 3

A

B
C
Si

18
Q

Why does mp drop from group 4 to 5

Why does mo increase from grp 1 to 3

A

Change from giant to simple structures

Nuclear charge increases so stronger electrostatic attraction in metallic bonding

19
Q

What is a reducing agent and example

Example of oxidising agent

A

Reduces other element but itself is oxidised
Eg metals

Eg halogens

20
Q

Why do trends in reactivity increase down grp 2

A

1st and 2nd ionisation energy decreases down grp so more reactive

21
Q

Product of grp 2 oxides and water

A

Unsaturated: metal and hydroxide ions in solution
Saturated: metal hydroxide solid

22
Q

Why does solubility of grp 2 increase down the group

A

Charge is same but mass increases so charge/mass ratio decreases so less electrostatic attraction and easier to pull apart

23
Q

Approx pH comparison of Mg(OH)2 and Ba(OH)2

A

Mg is 10
Ba is 13
Ba is more alkaline due to more OH- released in solution

24
Q

Grp 2 metal and acid product

A

Salt and hydrogen

25
Q

Grp 2 metal and water product

A

Metal hydroxide and hydrogen

26
Q

Use of grp 2 compounds in our lives

A

Agriculture: calcium hydroxide added to fields to decrease acidity of soil

Medicine: antacids, calcium carbonate react with HCl in stomach from indigestion

27
Q

Why does bp increase down group in halogens

A

Larger molecules so more electrons and stronger London forces so more energy needed to overcome intermolecular forces

28
Q

Why does reactivity decrease down halogens grp

A

Atomic radius/shielding increases so less nuclear attraction to attract an electron to join outer shell

29
Q

2 Disproportionation reactions of Cl

A

With low quantities of Cl2

1) With water forming HClO and HCl
2) With NaOH forming NaClO, NaCl and water

30
Q

Benefits and risks of Cl2 in water treatment

A

Bacteria killed so water borne diseases prevented

Cl2 gas is toxic and a respiratory irritant
Chlorinated hydrocarbons (methane from decaying vegetation) is a cancer risk if drank
31
Q

Explain displacement reaction amongst halogens

A

More reactive halogen will displace a less reactive one from a compound

32
Q

States at RTP of halogens

A 
In order down grp:
G
G
L
S
33
Q

Colour of halogens in water solution:
Cl2
Br2
I2

A

Pale green
Orange
Brown

34
Q

Colour of halogen in organic solvent (cyclohexane) solution
Cl2
Br2
I2

A

Pale green
Orange
Violet

35
Q

Why is cyclohexane added to halogen solution for identification/displacement reaction

A

Clearly differentiate between I2 and Br2 formation as both in water solution are similar in colour: orange vs brown
Difficult to tell apart depending on its conc

Chemistry (shubh) (9 decks)

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