Галогендер. Хлорсутек, тұз қышқылы және хлоридтер. Адам тіршілігіндегі йодтың биологиялық ролі. Йод жетіспеушілігінен туындайтын аурулардан Қазақстан тұрғындарын. Химия, 10 сынып, презентация.
Сабақ тақырыбы: Галогендер. Хлорсутек, тұз қышқылы және хлоридтер.
Адам тіршілігіндегі йодтың биологиялық ролі. Йод жетіспеушілігінен туындайтын аурулардан Қазақстан тұрғындарын
Оқу мақсаттары:
10.2.1.41 топ бойынша галогендердің физикалық және химиялық қасиеттерінің өзгеру заңдылығын түсіндіру;
10.2.1.42 тұз қышқылының химиялық қасиеттерін оқып білу және оның қолданылу аймағын білу;
10.4.1.12 адам ағзасындағы йодтың биологиялық ролін білу және Қазақстан территориясында йод жетіспеушілігіне байланысты туындайтын ауруларды түсіндіру және осы мәселелерді шешу жолын ұсыну;
At
Өткен сабақпен байланыс(W)
Мақсаты: Алдыңғы білімдерін еске түсіре отырып хлор элементінің атом құрылысымен танысу
Тапсырма.
Хлор атомының құрылысын жазып көрсетіңіз (протон, нейтрон, электрон саны, энергетикалық деңгей, конфигурация, графикалық формула, валентілігі, тотығу дәрежелері).
INTRODUCTION
F
Cl
Br
I
At
THE HALOGENS OCCUR IN GROUP XVII OF THE PERIODIC TABLE
Group 1 2 17
0
GROUP PROPERTIES
GENERAL • Бейметалл
• молекулалары екі атомнан тұрады…
мысалы Cl2
• соңғы қабатында 7 электрон болады
• иондары теріс зарядалған, аниондар, -1
GROUP PROPERTIES
GENERAL • non-metals
• exist as separate diatomic molecules… eg Cl2
• have seven electrons in their outer shells
• form negative ions with a 1- charge
• reaction with metals and halides
TRENDS • appearance сыртқы түрі
• boiling point қайнау нүктесі
• electronic configuration электрондық конфигурация
• atomic size атом өлшемі
• ionic size иондардың өлшемі
• reactivity белсенділігі
GROUP TRENDS
Топ өзгерісі
F2
Сары
Cl2
Жасыл
Br2
Қызыл қоңыр
I2
Сұр
ГАЗ
ГАЗ
СҰЙЫҚ
ҚАТТЫ
Colour
State (at RTP)
Сыртқы түрі
Сары
Жасыл
Қызыл қоңыр
Күлгін
Vapour colour
GROUP TRENDS
INCREASES down Group because more energy is required to separate the larger molecules.
Топ бойынша атомдық масса өскен сайын қайнау температурасы өседі, себебі молекулаларды үзуге көп энергия кетеді.
F2
Yellow
Cl2
Green
Br2
Red/brown
I2
Grey
GAS
GAS
LIQUID
SOLID
Colour
State (at RTP)
APPEARANCE
Қайнау температурасы
F2
- 188
Cl2
- 34
Br2
58
I2
183
Boiling point / °C
Yellow
Green
Red/brown
Purple
Vapour colour
GROUP TRENDS
F
Cl
Br
I
2,7
2,8,7
2,8,18,7
2,8,18,18,7
Configuration
Электрон конфигурациясы
9
17
35
53
Atomic Number
GROUP TRENDS
F
Cl
Br
I
атом & ион радиус
0.064
0.099
0.111
0.128
Atomic radius / nm
NOT TO SCALE
GROUP TRENDS
ATOMIC RADIUS INCREASES down Group
IONIC RADIUS INCREASES down Group
F
Cl
Br
I
атом & ион радиусы
0.064
0.099
0.111
0.128
Atomic radius / nm
F¯
Cl¯
Br¯
I¯
0.136
0.181
0.195
0.216
Ionic radius / nm
GROUP SIMILARITIES
GROUP SIMILARITIES
• all the atoms have seven electrons in their outer shell
• ions are larger than atoms - the added electron repels the
others so radius gets larger
ELECTRONIC CONFIGURATION
F
Cl
Br
I
2,7
2,8,7
2,8,18,7
2,8,18,18,7
Configuration
9
17
35
53
Atomic Number
GROUP SIMILARITIES
MOLECULAR FORMULA
F
Cl
Br
I
Covalent
Covalent
Covalent
Covalent
Bonding
F2
Cl2
Br2
I2
Molecular formula
NOT TO SCALE
• all exist as diatomic molecules
GROUP SIMILARITIES
ION FORMATION
F
Cl
Br
I
Configuration
Ion
F¯
Cl¯
Br¯
I¯
2,8
2,8,8
2,8,18,8
2,8,18,18,8
• all gain one electron to form a negative ion of charge 1-
• ions are larger than atoms
• the smaller the atom the easier it forms an ion
GROUP SIMILARITIES
ION FORMATION
F
Cl
Br
I
Configuration
Ion
F¯
Cl¯
Br¯
I¯
2,8
2,8,8
2,8,18,8
2,8,18,18,8
• all gain one electron to form a negative ion of charge 1-
• ions are larger than atoms
• the smaller the atom the easier it forms an ion
REACTIVITY
F
Cl
Br
I
Reactivity
Increasingly reactive
• reactivity decreases down the Group / increases up the Group
REACTIONS OF HALOGENS
1. WITH METALS
2. WITH HALIDES
REACTION OF HALOGENS WITH METALS
REACTION OF HALOGENS WITH METALS
HALOGENS REACT WITH METALS TO PRODUCE METAL HALIDES.
REACTION OF HALOGENS WITH METALS
HALOGENS REACT WITH METALS TO PRODUCE METAL HALIDES.
THE EASE OF REACTION DECREASES DOWN THE GROUP F > Cl > Br > I
REACTION OF HALOGENS WITH METALS
HALOGENS REACT WITH METALS TO PRODUCE METAL HALIDES.
THE EASE OF REACTION DECREASES DOWN THE GROUP F > Cl > Br > I
THIS IS BECAUSE ‘THE LARGER THE HALOGEN ATOM, THE LESS
EASILY IT ATTRACTS THE ELECTRON IT NEEDS
TO FILL ITS OUTER SHELL’
REACTION OF HALOGENS WITH METALS
HALOGENS REACT WITH METALS TO PRODUCE METAL HALIDES.
THE EASE OF REACTION DECREASES DOWN THE GROUP F > Cl > Br > I
THIS IS BECAUSE ‘THE LARGER THE HALOGEN ATOM, THE LESS
EASILY IT ATTRACTS THE ELECTRON IT NEEDS
TO FILL ITS OUTER SHELL’
THE HALIDES OF GROUP I ARE… WHITE IONIC SOLIDS
VERY SOLUBLE IN WATER
SODIUM CHLORIDE (NaCl) IS A TYPICAL GROUP I HALIDE
REACTION WITH ALKALI METALS
REACTION WITH ALKALI METALS - Equations
SODIUM CHLORINE SODIUM CHLORIDE
+
REACTION WITH ALKALI METALS - Equations
Na + Cl2 NaCl
SODIUM CHLORINE SODIUM CHLORIDE
REACTION WITH ALKALI METALS - Equations
Na + Cl2 NaCl
SODIUM CHLORINE SODIUM CHLORIDE
The equation doesn’t balance - multiply the formulae until it does
REACTION WITH ALKALI METALS - Equations
2Na + Cl2 2NaCl
Na + Cl2 NaCl
SODIUM CHLORINE SODIUM CHLORIDE
Balanced equation
Cl
SODIUM ATOM
2,8,1
Na
CHLORINE ATOM
2,8,7
11 protons; 11 electrons
17 protons; 17 electrons
SODIUM CHLORIDE FORMATION
Cl
SODIUM ION
2,8
Na
CHLORIDE ION
2,8,8
both species now have ‘full’ outer shells; ie they have the electronic configuration of a noble gas
+
11 protons; 10 electrons
17 protons; 18 electrons
SODIUM CHLORIDE FORMATION
Cl
SODIUM ION
2,8
Na
CHLORIDE ION
2,8,8
Na Na+ + e¯
2,8,1 2,8
ELECTRON TRANSFERRED
Cl + e¯ Cl¯
2,8,7 2,8,8
+
SODIUM CHLORIDE FORMATION
DISPLACEMENT REACTIONS OF HALOGENS
DISPLACEMENT REACTIONS OF HALOGENS
HALOGENS GET LESS REACTIVE AS THE GROUP IS DESCENDED
DISPLACEMENT REACTIONS OF HALOGENS
HALOGENS GET LESS REACTIVE AS THE GROUP IS DESCENDED
THIS DECREASE IN REACTIVITY DOWN THE GROUP CAN BE DEMONSTRATED USING DISPLACEMENT REACTIONS...
A DISPLACEMENT REACTION IS WHERE ONE SPECIES TAKES THE PLACE OF ANOTHER IN A COMPOUND.
DISPLACEMENT REACTIONS OF HALOGENS
HALOGENS GET LESS REACTIVE AS THE GROUP IS DESCENDED
THIS DECREASE IN REACTIVITY DOWN THE GROUP CAN BE DEMONSTRATED USING DISPLACEMENT REACTIONS...
A DISPLACEMENT REACTION IS WHERE ONE SPECIES TAKES THE PLACE OF ANOTHER IN A COMPOUND.
THE REACTIONS ARE EXAMPLES OF REDOX REACTIONS
DISPLACEMENT REACTIONS OF HALOGENS
SODIUM
CHLORIDE
SOLUTION
Colourless
SODIUM
BROMIDE
SOLUTION
Colourless
SODIUM
IODIDE
SOLUTION
Colourless
CHLORINE
WATER
Pale green
BROMINE
WATER
Orange
A SOLUTION OF THE HALOGEN IS ADDED TO A SOLUTION OF A HALIDE
HALIDES ARE SALTS FORMED BETWEEN ELEMENTS AND HALOGENS
DISPLACEMENT REACTIONS OF HALOGENS
SODIUM
BROMIDE
SOLUTION
Colourless
SODIUM
IODIDE
SOLUTION
Colourless
CHLORINE
WATER
Pale green
BROMINE
WATER
Orange
SODIUM
CHLORIDE
SOLUTION
Colourless
NO VISIBLE REACTION
Experiment 1
DISPLACEMENT REACTIONS OF HALOGENS
SODIUM
CHLORIDE
SOLUTION
Colourless
SODIUM
IODIDE
SOLUTION
Colourless
BROMINE
WATER
Orange
CHLORINE
WATER
Pale green
SODIUM
BROMIDE
SOLUTION
Colourless
BROMINE produced
Experiment 2
DISPLACEMENT REACTIONS OF HALOGENS
SODIUM
CHLORIDE
SOLUTION
Colourless
SODIUM
BROMIDE
SOLUTION
Colourless
BROMINE
WATER
Orange
CHLORINE
WATER
Pale green
SODIUM
IODIDE
SOLUTION
Colourless
IODINE produced
Experiment 3
DISPLACEMENT REACTIONS OF HALOGENS
SODIUM
BROMIDE
SOLUTION
Colourless
SODIUM
IODIDE
SOLUTION
Colourless
CHLORINE
WATER
Pale green
BROMINE
WATER
Orange
SODIUM
CHLORIDE
SOLUTION
Colourless
NO VISIBLE REACTION
Experiment 4
DISPLACEMENT REACTIONS OF HALOGENS
SODIUM
CHLORIDE
SOLUTION
Colourless
SODIUM
IODIDE
SOLUTION
Colourless
CHLORINE
WATER
Pale green
BROMINE
WATER
Orange
SODIUM
BROMIDE
SOLUTION
Colourless
NO VISIBLE REACTION
Experiment 5
DISPLACEMENT REACTIONS OF HALOGENS
SODIUM
CHLORIDE
SOLUTION
Colourless
SODIUM
BROMIDE
SOLUTION
Colourless
CHLORINE
WATER
Pale green
BROMINE
WATER
Orange
SODIUM
IODIDE
SOLUTION
Colourless
IODINE produced
Experiment 6
SODIUM CHLORIDE
CHLORINE
SODIUM BROMIDE
SODIUM IODIDE
Solution stays colourless
NO REACTION
Solution goes from colourless to orange-yellow
NO REACTION
Solution goes from colourless to orange-yellow
BROMINE FORMED
Solution goes from colourless to orange-yellow
NO REACTION
Solution goes from colourless to red
IODINE FORMED
BROMINE
Solution goes from colourless to orange-red
IODINE FORMED
DISPLACEMENT REACTIONS OF HALOGENS
SUMMARY OF OBSERVATIONS
1
6
5
2
3
4
The colour change in Experiments 4 and 5 is due to dilution – there is no reaction
CHLORINE + SODIUM BROMIDE
CHLORINE + SODIUM IODIDE
BROMINE + SODIUM IODIDE
DISPLACEMENT REACTIONS OF HALOGENS
EQUATIONS
CHLORINE + SODIUM BROMIDE BROMINE + SODIUM CHLORIDE
CHLORINE + SODIUM IODIDE IODINE + SODIUM CHLORIDE
BROMINE + SODIUM IODIDE IODINE + SODIUM BROMIDE
DISPLACEMENT REACTIONS OF HALOGENS
EQUATIONS
CHLORINE + SODIUM BROMIDE BROMINE + SODIUM CHLORIDE
CHLORINE + SODIUM IODIDE IODINE + SODIUM CHLORIDE
BROMINE + SODIUM IODIDE IODINE + SODIUM BROMIDE
DISPLACEMENT REACTIONS OF HALOGENS
EQUATIONS
Cl2(aq) + NaBr(aq) —> Br2(aq) + NaCl(aq)
The equation doesn’t balance - multiply the formulae until it does
CHLORINE + SODIUM BROMIDE BROMINE + SODIUM CHLORIDE
CHLORINE + SODIUM IODIDE IODINE + SODIUM CHLORIDE
BROMINE + SODIUM IODIDE IODINE + SODIUM BROMIDE
DISPLACEMENT REACTIONS OF HALOGENS
EQUATIONS
Cl2(aq) + 2NaBr(aq) —> Br2(aq) + 2NaCl(aq)
Cl2(aq) + NaBr(aq) —> Br2(aq) + NaCl(aq)
CHLORINE + SODIUM BROMIDE BROMINE + SODIUM CHLORIDE
CHLORINE + SODIUM IODIDE IODINE + SODIUM CHLORIDE
BROMINE + SODIUM IODIDE IODINE + SODIUM BROMIDE
DISPLACEMENT REACTIONS OF HALOGENS
EQUATIONS
Cl2(aq) + 2Br¯(aq) —> Br2(aq) + 2Cl¯(aq)
Cl2(aq) + 2NaBr(aq) —> Br2(aq) + 2NaCl(aq)
IONIC EQUATION
CHLORINE + SODIUM BROMIDE BROMINE + SODIUM CHLORIDE
CHLORINE + SODIUM IODIDE IODINE + SODIUM CHLORIDE
BROMINE + SODIUM IODIDE IODINE + SODIUM BROMIDE
DISPLACEMENT REACTIONS OF HALOGENS
EQUATIONS
Cl2(aq) + 2I¯(aq) —> I2(aq) + 2Cl¯(aq)
Cl2(aq) + 2NaI(aq) —> I2(aq) + 2NaCl(aq)
IONIC EQUATION
CHLORINE + SODIUM BROMIDE BROMINE + SODIUM CHLORIDE
CHLORINE + SODIUM IODIDE IODINE + SODIUM CHLORIDE
BROMINE + SODIUM IODIDE IODINE + SODIUM BROMIDE
DISPLACEMENT REACTIONS OF HALOGENS
EQUATIONS
Br2(aq) + 2I¯(aq) —> I2(aq) + 2Br¯(aq)
Br2(aq) + 2NaI(aq) —> I2(aq) + 2NaBr(aq)
IONIC EQUATION
CHLORINE + SODIUM BROMIDE BROMINE + SODIUM CHLORIDE
CHLORINE + SODIUM IODIDE IODINE + SODIUM CHLORIDE
BROMINE + SODIUM IODIDE IODINE + SODIUM BROMIDE
THIS SHOWS THAT A MORE REACTIVE HALOGEN WILL DISPLACE
A LESS REACTIVE ONE FROM AN AQUEOUS SOLUTION OF ITS SALT
DISPLACEMENT REACTIONS OF HALOGENS
SUMMARY
CHLORINE + SODIUM BROMIDE BROMINE + SODIUM CHLORIDE
CHLORINE + SODIUM IODIDE IODINE + SODIUM CHLORIDE
BROMINE + SODIUM IODIDE IODINE + SODIUM BROMIDE
THIS SHOWS THAT A MORE REACTIVE HALOGEN WILL DISPLACE
A LESS REACTIVE ONE FROM AN AQUEOUS
SOLUTION OF ITS SALT
HOWEVER, THIS REACTION DOES NOT TAKE PLACE
BROMINE + SODIUM CHLORIDE CHLORINE + SODIUM BROMIDE
(Bromine is below chlorine in the Group so is less reactive)
DISPLACEMENT REACTIONS OF HALOGENS
EQUATIONS
PRESS THE SPACE BAR TO SEE WHAT HAPPENS
DISPLACEMENT REACTIONS OF HALOGENS
EXPLANATION
17+
CHLORINE ATOM
17 PROTONS
17 ELECTRONS
2,8,7
35+
BROMIDE ION
35 PROTONS
36 ELECTRONS
2,8,18,8
THE CHLORINE ATOM PULLS AN ELECTRON OUT OF THE OUTER SHELL OF THE BROMIDE ION – THE CHLORINE ATOM BECOMES A CHLORIDE ION AND THE BROMIDE ION BECOMES A BROMINE ATOM.
BECAUSE BROMINE ATOMS ARE LARGER THAN CHLORINE ATOMS, IT IS EASIER TO PULL ONE OF THEIR OUTER SHELL ELECTRONS OUT.
CHLORINE NOW HAS THE OUTER SHELL ELECTRONIC CONFIGURATION OF A NOBLE GAS.
DISPLACEMENT REACTIONS OF HALOGENS
EXPLANATION
CHLORINE ATOM
17 PROTONS
17 ELECTRONS
BROMIDE ION
35 PROTONS
36 ELECTRONS
DISPLACEMENT REACTIONS OF HALOGENS - REDOX
A REDOX REACTION INVOLVES BOTH OXIDATION AND REDUCTION
DISPLACEMENT REACTIONS OF HALOGENS - REDOX
A REDOX REACTION INVOLVES BOTH OXIDATION AND REDUCTION
REDUCTION IS THE… GAIN OF ELECTRONS
OXIDATION IS THE… REMOVAL OF ELECTRONS
DISPLACEMENT REACTIONS OF HALOGENS - REDOX
A REDOX REACTION INVOLVES BOTH OXIDATION AND REDUCTION
REDUCTION IS THE… GAIN OF ELECTRONS
OXIDATION IS THE… REMOVAL OF ELECTRONS
IN THE REACTION BETWEEN CHLORINE AND SODIUM BROMIDE, CHLORINE ATOMS PULL ELECTRONS OUT OF BROMIDE IONS.
DISPLACEMENT REACTIONS OF HALOGENS - REDOX
Cl2(aq) + 2Br¯(aq) ——> Br2(aq) + 2Cl¯(aq)
A REDOX REACTION INVOLVES BOTH OXIDATION AND REDUCTION
REDUCTION IS THE… GAIN OF ELECTRONS
OXIDATION IS THE… REMOVAL OF ELECTRONS
IN THE REACTION BETWEEN CHLORINE AND SODIUM BROMIDE, CHLORINE ATOMS PULL ELECTRONS OUT OF BROMIDE IONS.
THE BROMIDE IONS ARE OXIDISED… ELECTRONS ARE REMOVED
DISPLACEMENT REACTIONS OF HALOGENS - REDOX
Cl2(aq) + 2Br¯(aq) ——> Br2(aq) + 2Cl¯(aq)
OXIDISED
ELECTRONS
REMOVED
CHLORINE IS THE OXIDISING AGENT
A REDOX REACTION INVOLVES BOTH OXIDATION AND REDUCTION
REDUCTION IS THE… GAIN OF ELECTRONS
OXIDATION IS THE… REMOVAL OF ELECTRONS
IN THE REACTION BETWEEN CHLORINE AND SODIUM BROMIDE, CHLORINE ATOMS PULL ELECTRONS OUT OF BROMIDE IONS.
THE BROMIDE IONS ARE OXIDISED… ELECTRONS ARE REMOVED
THE CHLORINE ATOMS ARE REDUCED… ELECTRONS ARE GAINED
DISPLACEMENT REACTIONS OF HALOGENS - REDOX
Cl2(aq) + 2Br¯(aq) ——> Br2(aq) + 2Cl¯(aq)
REDUCED
GAIN OF ELECTRONS
BROMIDE ION IS THE REDUCING AGENT
A REDOX REACTION INVOLVES BOTH OXIDATION AND REDUCTION
REDUCTION IS THE… GAIN OF ELECTRONS
OXIDATION IS THE… REMOVAL OF ELECTRONS
IN THE REACTION BETWEEN CHLORINE AND SODIUM BROMIDE, CHLORINE ATOMS PULL ELECTRONS OUT OF BROMIDE IONS.
THE BROMIDE IONS ARE OXIDISED… ELECTRONS ARE REMOVED
THE CHLORINE ATOMS ARE REDUCED… ELECTRONS ARE GAINED
DISPLACEMENT REACTIONS OF HALOGENS - REDOX
Cl2(aq) + 2Br¯(aq) ——> Br2(aq) + 2Cl¯(aq)
REDUCED
OXIDISED
ELECTRONS
REMOVED
GAIN OF ELECTRONS
OXIDISING POWER OF HALOGENS
HALOGENS GET LESS REACTIVE AS THE GROUP IS DESCENDED
THIS IS DUE TO THEIR DECREASING OXIDISING ABILITY
OXIDISING POWER OF HALOGENS
HALOGENS GET LESS REACTIVE AS THE GROUP IS DESCENDED
THIS IS DUE TO THEIR DECREASING OXIDISING ABILITY
F
Cl
Br
I
2,7
2,8,7
2,8,18,7
2,8,18,18,7
Configuration
9
17
35
53
Atomic Number
0.064
0.099
0.111
0.128
Atomic radius / nm
---- DECREASING OXIDISING POWER ----->
OXIDISING POWER OF HALOGENS
HALOGENS GET LESS REACTIVE AS THE GROUP IS DESCENDED
THIS IS DUE TO THEIR DECREASING OXIDISING ABILITY
F
Cl
Br
I
2,7
2,8,7
2,8,18,7
2,8,18,18,7
Configuration
9
17
35
53
Atomic Number
0.064
0.099
0.111
0.128
Atomic radius / nm
THE SMALLER THE HALOGEN, THE LESS SHIELDING THERE IS AND THE GREATER THE EFFECTIVE PULL OF THE NUCLEUS.
---- DECREASING OXIDISING POWER ----->
OXIDISING POWER OF HALOGENS
HALOGENS GET LESS REACTIVE AS THE GROUP IS DESCENDED
THIS IS DUE TO THEIR DECREASING OXIDISING ABILITY
F
Cl
Br
I
2,7
2,8,7
2,8,18,7
2,8,18,18,7
Configuration
9
17
35
53
Atomic Number
0.064
0.099
0.111
0.128
Atomic radius / nm
THE SMALLER THE HALOGEN, THE LESS SHIELDING THERE IS AND THE GREATER THE EFFECTIVE PULL OF THE NUCLEUS.
THE GREATER THE PULL OF THE NUCLEUS, THE EASIER THE ATOM CAN PULL AN ELECTRON OUT OF ANOTHER SPECIES.
---- DECREASING OXIDISING POWER ----->
OXIDISING POWER OF HALOGENS
HALOGENS GET LESS REACTIVE AS THE GROUP IS DESCENDED
THIS IS DUE TO THEIR DECREASING OXIDISING ABILITY
F
Cl
Br
I
2,7
2,8,7
2,8,18,7
2,8,18,18,7
Configuration
9
17
35
53
Atomic Number
0.064
0.099
0.111
0.128
Atomic radius / nm
THE SMALLER THE HALOGEN, THE LESS SHIELDING THERE IS AND THE GREATER THE EFFECTIVE PULL OF THE NUCLEUS.
THE GREATER THE PULL OF THE NUCLEUS, THE EASIER THE ATOM CAN PULL AN ELECTRON OUT OF ANOTHER SPECIES.
CONSEQUENTLY, THE BIGGER THE ATOM, THE EASIER AN ELECTRON CAN BE REMOVED.
---- DECREASING OXIDISING POWER ----->
SYMBOL
MOLECULAR FORMULA
APPEARANCE
STATE (room temp)
F
PALE YELLOW
GAS
Cl
FLUORINE
IODINE
ELECTRONIC CONFIGURATION
BOILING POINT
2,7
INCREASES
2,8,7
GAS
ION
(electronic config)
F¯
2,8
Cl¯
2,8,8
REACTION WITH SODIUM
LESS REACTIVE
PRODUCT OF REACTION WITH SODIUM
SODIUM FLUORIDE (NaF)
SODIUM CHLORIDE (NaCl)
PALE GREEN
Br
I
BROMINE
CHLORINE
F2
Cl2
Br2
I2
RED-BROWN
GREY-BLACK
LIQUID
SOLID
2,8,18,7
2,8,18,18,7
Br¯
2,8,18,8
I¯
2,8,18,18,8
SODIUM BROMIDE (NaBr)
SODIUM IODIDE (NaI)
GROUP VII - SUMMARY
COLOUR OF VAPOUR
PALE YELLOW
GREEN
RED-BROWN
PURPLE
QUICK QUIZ
ELEMENTS IN GROUP 7 ARE KNOWN AS THE ………
WHAT ARE THE NAMES OF THE ELEMENTS
HOW DOES THE ATOMIC NUMBER CHANGE DOWN THE GROUP?
HOW DOES THE ELECTRONIC CONFIGURATION CHANGE?
HOW DOES THE ATOMIC SIZE (RADIUS) CHANGE?
HOW MANY ELECTRONS DO THEY HAVE IN THE OUTER LEVEL?
ARE THEY METALS OR NON-METALS?
WHAT HAPPENS TO THEIR COLOUR DOWN THE GROUP?
DO THEY GO AROUND IN PAIRS OR AS MONATOMIC GASES?
WHAT HAPPENS TO THEIR STATE AT ROOM TEMPERATURE?
WHAT TYPE OF COMPOUNDS DO THEY FORM WITH METALS?
HOW CAN EXPLAIN THEIR RELATIVE REACTIVITY IN TERMS OF THE ATOMIC STRUCTURE?
QUICK QUIZ - ANSWERS
HALOGENS.
FLUORINE, CHLORINE, BROMINE, IODINE, ASTATINE.
ATOMIC NUMBER INCREASES DOWN THE GROUP.
GET MORE SHELLS DOWN THE GROUP.
ATOMIC SIZE INCREASES DOWN THE GROUP.
THEY ALL HAVE SEVEN ELECTRONS IN THE OUTER LEVEL.
THEY ARE NON-METALS.
COLOUR DARKENS DOWN THE GROUP.
ATOMS GO AROUND IN PAIRS OR AS DIATOMIC GASES.
GO FROM GAS TO SOLID DOWN THE GROUP.
THEY FORM IONIC COMPOUNDS WITH METALS.
THE LARGER THEY ARE THE LESS EASILY ELECTRONS ARE GAINED AND THE LESS REACTIVE THEY BECOME.
HYDROGEN CHLORIDE OR HYDROCHLORIC ACID?
HYDROGEN CHLORIDE OR HYDROCHLORIC ACID?
Hydrogen chloride is a colourless covalent gas; it is a poor conductor of electricity because there are no free electrons or ions present. It has no action on dry litmus paper because there are no aqueous hydrogen ions present.
Hydrogen chloride is a colourless covalent gas; it is a poor conductor of electricity because there are no free electrons or ions present. It has no action on dry litmus paper because there are no aqueous hydrogen ions present.
HYDROGEN CHLORIDE OR HYDROCHLORIC ACID?
Hydrogen chloride is a colourless covalent gas; it is a poor conductor of electricity because there are no free electrons or ions present. It has no action on dry litmus paper because there are no aqueous hydrogen ions present.
In water, the hydrogen chloride molecules dissociate into ions. The solution now conducts electricity showing ions are present. For each hydrogen chloride molecule that dissociates (splits up) one hydrogen ion and one chloride ion are produced. The solution turns litmus paper red because of the H+(aq) ions.
HYDROGEN CHLORIDE OR HYDROCHLORIC ACID?
HYDROGEN CHLORIDE HYDROCHLORIC ACID
colourless gas Appearance colourless soln.
covalent molecule Bonding aqueous ions
HCl(g) Formula HCl(aq)
poor Conductivity good
no reaction Dry blue litmus goes red
HYDROGEN CHLORIDE OR HYDROCHLORIC ACID?
HCl(g) —> H+ (aq) + Cl¯(aq)
Hydrogen chloride dissociates in water because water is a polar solvent. However, when hydrogen chloride is placed in an organic solvent such as methylbenzene it does not dissociate and does not produce H+ ions.
WATER
A polar solvent
Molecules dissociate
The solution turns litmus paper red because of the H+(aq) ions.
DOES HYDROGEN CHLORIDE ALWAYS DISSOCIATE?
METHYLBENZENE
A non-polar solvent
NO dissociation
The solution does not litmus paper red because there are NO H+(aq) ions.
WATER IS A POLAR SOLVENT –
it has one end which is slightly positive and another end which is slightly positive.
WHY DOES HYDROGEN CHLORIDE DISSOCIATE IN WATER?
positive end
negative end
WATER IS A POLAR SOLVENT –
it has one end which is slightly positive and another end which is slightly positive.
WHY DOES HYDROGEN CHLORIDE DISSOCIATE IN WATER?
When a molecule of hydrogen chloride is put into water, the water molecules ‘encourage’ the covalent bond holding the hydrogen and chlorine atoms together to split, thus forming ions.
positive end
negative end
HCl(g) —> H+ (aq) + Cl¯(aq)
WHY DOES HYDROGEN CHLORIDE DISSOCIATE IN WATER?
The chloride ions are attracted to the slightly positive hydrogen end of water.
The slightly negative oxygen end of water attracts the H+ ions.
When a molecule of hydrogen chloride is put into water, the water molecules ‘encourage’ the covalent bond holding the hydrogen and chlorine atoms together to split, thus forming ions.
HCl(g) —> H+ (aq) + Cl¯(aq)
WATER IS A POLAR SOLVENT –
it has one end which is slightly positive and another end which is slightly positive.
positive end
negative end
GROUP VII
The Halogens
THE END
© 2011 KNOCKHARDY PUBLISHING & JONATHAN HOPTON
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