Shadowing Practice: GENERAL CHEMISTRY explained in 19 Minutes - Learn English Speaking with Video
Bir pratik modu seçin
Her mod tam ekran bir pratik odası açar.
298 cümleler
Cümleler çok kısa veya çok uzun ise, ayarlamak için Düzenle'ye tıklayın.
1
Everything is made of atoms.
2
Yes, even you.
3
Atoms consist of a core and some electrons.
4
The core is made of protons and neutrons, and depending on the number of protons, you get different elements.
5
Water is made of hydrogen and oxygen.
6
This is some sodium.
7
Hmm, I wonder what happens when you...
8
Ha, whoopsie.
9
Quantum mechanics tells us that this is not what atoms actually look like.
10
They look more like this, but we'll get to that later.
11
For now, just think of atoms as having multiple electron shells.
12
The electrons in the outermost shell are called valence electrons.
13
Most of chemistry is really just the behavior of these electrons.
14
Every element is listed in the periodic table.
15
All elements in the same column or group have the same number of valence electrons.
16
For the main groups, the number of valence electrons is just the group number from 1 to 8.
17
Except for helium.
18
It's too small to have 8 electrons, it can only have 2, but still, it acts like a noble gas,
19
so it's just kinda grouped in with those.
20
Luckily, the transition metals also follow a nice pattern.
21
That was a lie, it's kind of a mess, but that's not so important for now, so we'll get to that later.
22
Elements with the same number of valence electrons tend to show similar behavior in chemical reactions.
23
For example, the first group without hydrogen is called the alkali metals.
24
Here's some things they have in common.
25
They have one valence electron, they're shiny metals, they're kind of soft, and they do this sometimes.
26
All elements in the same row or period have the same number of shells.
27
This number increases from top to bottom.
28
Also, the mass gets bigger from left to right, as each element gains a proton, an electron, and some neutrons.
29
Depending on the number of neutrons in the core, you get different isotopes of the same element,
30
most of which are pretty unstable and fall apart, releasing ionizing radiation.
31
Fun fact, that stuff will kill you.
32
If an atom has the same amount of electrons as protons, it has no charge.
33
If it has more, it has a negative charge, and if it has less, it has a positive charge.
34
Charged atoms are called ions.
35
Negative ions are anions, and positive ions are cations.
36
The periodic table is also pretty much a dictionary, as every cell tells you the name and symbol of an element,
37
the number of protons in the core, which is also the total number of electrons,
38
and the atomic mass, which is the mass of neutrons and protons combined.
39
The periodic table is roughly divided into three categories.
40
Left of this line are the metals, right of it are the non -metals, which are mostly gases, and the line is called the semi -metals,
41
which have properties that fall somewhere in between.
42
Two or more atoms bonded together form a molecule.
43
If you have at least two different elements, you get a compound.
44
Oh yeah, this is probably a good time to mention that compounds often behave completely differently than the elements they're made of.
45
Like you put together an explosive metal and a toxic gas, and you get, of course, an even more expli - Table salt.
46
You get table salt.
47
There's many ways to write molecules, for example the molecular formula, where you just count the number of each atom in a molecule
48
and write them as a subscript number next to the element symbol.
49
But that has some problems, look at these two molecules.
50
They have the same molecular formula, but obviously they're not the same.
51
They're isomers.
52
Showing this difference is probably kind of important, it's the only thing that separates graphite from diamonds, because they're both just fancy versions of carbon,
53
and I don't think anyone's gonna go, well, yes, this dusty black blob is indeed very expensive.
54
One way to show the structure of an atom is a Lewis dot structure, which represents the valence electrons and bonds as dots and lines.
55
This is also going to help us understand why atoms bond in the first place.
56
You see, everything in the universe wants to get to a state of lower energy.
57
That's why a ball on a hill will roll down by itself, because that decreases its potential energy.
58
This trend also applies to atoms.
59
The state of lowest potential energy is having a full outer shell of electrons, which is most often eight,
60
or in the case of hydrogen and helium, too.
61
If you think back to the periodic table, you'll see that all noble gases already have a full outer shell,
62
which is why they don't really want to react with anything.
63
If two atoms don't have a full outer shell, but can achieve one by sharing electrons, they will naturally do so,
64
the same way a ball will go downhill, as their combined energy would be lower than if they were separate.
65
The sharing of electrons is called a covalent bond.
66
These bonds are also caused by the positively charged nucleus of an atom tugging on electrons of another atom.
67
The strength of this pole is called electronegativity.
68
In the periodic table, the electronegativity increases from bottom left to the top right.
69
Therefore, fluorine has the strongest pull.
70
It's just unbelievably desperate for an electron.
71
If the difference in electronegativity is bigger than about 1 .7, you get an ionic bond.
72
A good example is sodium chloride.
73
Chlorine would do anything for an electron, while sodium has one too many and just kinda wants to get rid of it anyway.
74
Perfect, they both say, forming an ionic bond, where sodium loses an electron and turns into a cation,
75
and chlorine gains an electron and turns into an anion.
76
That seems pretty important.
77
You might want to remember it.
78
The most common place you see ionic bonds is in salt.
79
Yes, also table salt, but more generally when metals and non -metals bond you get a salt, which is just a grid of ions.
80
Speaking of metals, a pure metal forms metallic bonds.
81
You can imagine this as a huge grid of positively charged nuclei, which are surrounded by freely moving electrons.
82
You see, in a metal grid, the valence electrons are kinda promiscuous, or as the nerds call it, delocalized.
83
They can move freely in a giant playground of nuclei instead of being loyal to just one.
84
This kind of bond is responsible for the properties of metals, like conducting electricity and heat, and also being malleable, as in being kind of bendy.
85
Like, you can hammer on this stuff until it's the most deformed, unelegant, and ugly -looking piece of material ever known,
86
and it will just limp along as if nothing ever happened.
87
If the difference in electronegativity is lower than about 0 .5, the electrons are shared pretty equally and you get a non -polar covalent bond.
88
If it's bigger than 0 .5 but smaller than around 1 .7, one of the elements is pulling on the electrons pretty hard.
89
Not quite hard enough to completely steal an electron, but definitely hard enough to skew the electrons a bit, making it a polar covalent bond.
90
An example is water.
91
Oxygen has a very high electronegativity compared to hydrogen.
92
As a result, it pulls the electrons of hydrogen so hard that they kind of belong to oxygen, giving it a partial negative charge,
93
and leaving hydrogen with a partial positive charge.
94
The presence of two poles with opposite charge is called an electric dipole.
95
All permanent dipole molecules can interact with each other, and really with anything that has a charge.
96
As a result, the molecules will tug on each other
97
and arrange themselves in a way that oppositely charged ends are next to each other.
98
The forces acting between them are called intermolecular forces, or IMFs.
99
A specific example is hydrogen bonds, where hydrogen bonds to something very electronegative, like fluorine, oxygen, or nitrogen, creating strong dipoles that tug on each other.
100
But even if molecules are not polar at all, there can be electrostatic forces acting between them.
101
How?
102
Electrons move around inside the atoms, and by pure chance they can end up on one side of the atom,
103
creating a momentary dipole, which influences other particles next to it to become a dipole as well.
104
At least for a very short time, as the electrons keep moving and the dipole disappears.
105
This is called the van der Waals forces.
106
The polarity of water also explains why it's one of the most versatile solvents to exist.
107
It can pull apart molecules by tugging on charges, and it keeps them apart by surrounding a particle with its oppositely charged end.
108
Water cannot dissolve non -polar molecules though.
109
It's the reason why water and oil don't mix, since fat molecules are non -polar while water is polar.
110
Just remember the ancient saying, Similia similibus solventum.
111
Or in the language that's actually spoken, similar things will dissolve similar things things.
112
Fun fact!
113
Soap works because the molecules that it's made from, which are called surfactants, have a polar head and a nonpolar tail.
114
This way, when in water, they can surround for example nonpolar fat molecules and form micelles, which along with the water, transport the dirt particles away.
115
These are the most important bonds and forces ranked by strength.
116
Ionic bonds, covalent bonds, metallic bonds, hydrogen bonds, and van der Waals forces.
117
There are three main states of matter.
118
Solid, liquid, and gas.
119
Solids are tightly packed in fixed structures, where the particles can only wiggle.
120
Unless, you know, you smash them.
121
In liquids, the particles can move freely but are still confined to a fixed volume,
122
as the forces between them are still strong enough to keep them together.
123
And the particles and gases have enough energy to just do whatever they want
124
and fill up all the volume you give them.
125
Knowing this, we can find two important words.
126
Temperature is the average kinetic energy of particles in a system, or how much and how fast they move, and entropy is the amount of disorder.
127
Substances tend to be solid at low temperature and or high pressure, which is a state of low entropy,
128
as they're neatly organized and don't move that much, and gas at a high temperature and or low pressure,
129
where they move around like crazy so it's a state of high entropy.
130
Strong bonds like ionic bonds lead to high melting points, as they take a lot of energy and therefore a high temperature to break apart.
131
That's why most salts are solid at room temperature, whereas water, which is only being held together by hydrogen bonds, is a liquid.
132
Well actually, there's another state called plasma,
133
which is ionized gas and can exist at very high temperatures such as in stars or very high electric potential.
134
The latter is used for neon lights.
135
Gas is ionized in a tube with a very high voltage.
136
Collisions of the ions with other particles makes their electrons move to a higher energy state.
137
Once they fall back down, the difference in energy is released as light.
138
The color of the light depends on the element that's used in the tube, as each element has different but fixed energy levels,
139
and the difference between those determines the energy and therefore the frequency of the released light, which is what changes the color.
140
All possible frequencies that an element can emit are called the emission spectrum.
141
All matter can be divided into two categories pure substances, which can consist of one element or one compound, and mixtures.
142
Mixtures consist of at least two pure substances and can be homogeneous or heterogeneous.
143
Homogeneous means the substances we'll mix evenly and the mixture looks the same everywhere, like salt and water, which is a solution.
144
Heterogeneous mixtures look different depending on where you look.
145
They have distinct regions made of separate substances.
146
One example is sand and water, which is called a suspension.
147
Okay, well what about milk?
148
That looks the same everywhere, so it must be homogeneous.
149
Uh, no, milk is something we call a colloid, or more precisely, an emulsion.
150
The difference between salt water and milk is that the solute doesn't fully dissolve in the solvent, meaning there are bigger particles than in a solution,
151
but smaller particles than in a suspension.
152
This allows the particles to stay evenly distributed, but not fully dissolved, placing them somewhere between solutions and suspensions.
153
Hey, remember sodium and water?
154
What's going on there?
155
Explosions are really just chemical reactions that release a lot of energy in a very short amount of time.
156
Also, they expand.
157
Like, a lot.
158
There's a couple types of chemical reactions.
159
Synthesis, decomposition, signal replacement, and double replacement.
160
Here's an example for each one.
161
They all happen mainly for one reason, to decrease energy and get to a more stable state.
162
Chemical reactions happen in certain ratios.
163
For example, to produce water molecules you need twice the amount of hydrogen compared to oxygen.
164
This is called stoichiometry.
165
These ratios are based on the conservation of mass, which says that mass cannot be created or destroyed, only converted.
166
Practically, when dealing with reaction equations, you have to make sure that there's the same amount of atoms on each side of the equation,
167
and if not, balance it out element by element.
168
As a rule of thumb, you should balance out the metals first, then the non -metals, and then hydrogen and oxygen at the end.
169
But it's really just trial and error until everything is balanced.
170
Okay, but if you wanted to make this reaction happen in a lab,
171
how would we know that we have exactly twice the amount of hydrogen compared to oxygen?
172
You can't just take 10 grams of this and mix it with 20 grams of that, because the atoms don't weigh the same,
173
so 10 grams of both contain a different amount of particles.
174
What to do?
175
Just look up the atomic mass of the reactants and take that amount in grams.
176
You'll get exactly this amount of particles.
177
That is one mole, which is just an amount of something, kind of like a dozen.
178
In other words, we can interpret the reaction as two moles of this react with one mole of that, which we can easily measure.
179
It's important to differentiate between physical and chemical changes, as reactions only take place in the latter.
180
Physical change happens when the appearance changes, but the substance does not.
181
For example, hammering metal.
182
A chemical change happens when the substances themselves change, and this is often accompanied by bubbles, a funky smell, or, you guessed it, explosions.
183
All chemical reactions need activation energy to take place.
184
Wood won't just spontaneously react with oxygen and start burning, or else, you know, the planet would be on fire,
185
but if you give it enough energy, it will.
186
Catalysts reduce the activation energy needed for a reaction, which makes it happen easier and faster.
187
And as a neat bonus, they don't even get used up during the reaction so you can just reuse them.
188
Because chemical reactions are changes in energy, it's quite useful to keep track of it.
189
Enthalpy is, simply put, the internal energy or heat content of a system.
190
If the total enthalpy of a reaction is lower at the end than at the beginning, heat was given off to the surroundings,
191
which is an exothermic reaction.
192
If it's the other way around, a reaction is endothermic.
193
It's easy to see how exothermic reactions can be spontaneous.
194
It's kind of like a ball on a hill.
195
It will only start rolling if you push it a little bit, but then it will keep rolling on its own.
196
Just like wood keeps burning on its own.
197
But in endothermic reactions, you have to keep putting in energy, like pushing a ball uphill.
198
That doesn't just spontaneously happen, right?
199
Well, yes, actually it does.
200
To get the whole picture, we have to look at Gibbs free energy, which looks at the change of enthalpy,
201
but also the entropy of a system, which is dependent on temperature.
202
If this whole thing is less than zero, the reaction is exergonic, or spontaneous, because free energy was released.
203
If it's bigger than zero, it's endogonic, or not spontaneous, because free energy was needed and absorbed.
204
Here's where temperature and entropy come into play.
205
Even if delta H is positive, so the reaction is endothermic, if the change in entropy is big enough,
206
it can offset this and make the total free energy negative, which means the reaction is spontaneous.
207
But this is strongly dependent on the temperature.
208
For example, melting an ice cube is endothermic, because it absorbs heat.
209
But also, it increases the entropy a lot, as neatly organized ice turns into water, which is just kind of a mess.
210
So this can happen spontaneously, but only if the temperature is above zero.
211
If it's below zero, the water will spontaneously freeze, which is exothermic.
212
If it's exactly zero, then no reaction will take place spontaneously.
213
In other words, if delta G is zero, we're at equilibrium.
214
Chemical equilibriums exist when reversible reactions take place at the same speed in both directions, which means that even if reactions are taking place,
215
the concentrations of both sides stay the same, and to someone watching from the outside, nothing seems to be happening.
216
We often find chemical equilibriums in phase changes, but also acid -base chemistry.
217
According to Branstad -Lowry, an acid is a molecule that donates protons, while bases accept protons.
218
A proton in this case is just a hydrogen ion.
219
So, with this definition, a molecule with at least one hydrogen that it can throw away can be an acid,
220
and anything that can pick it up can be a base.
221
This also means that once they react, they turn into the conjugate opposite, as an acid that gave away a proton can now accept one back,
222
which is what bases do.
223
A molecule that can act as both an acid and a base is amphoteric, for example water.
224
A strong acid will dissociate almost completely into its ionic form,
225
giving off a lot of protons to the water and therefore creating lots of hydronium ions.
226
A weak acid just won't dissociate nearly as much, giving us a lower concentration of hydronium ions.
227
So, to measure the strength of an acid we can measure the concentration of hydronium ions.
228
This is called the pH.
229
Mathematically, it's defined as the negative log of the hydronium concentration, which means one step on the scale is a 10 times change,
230
and also, since it's a negative log, the higher the concentration, the lower the pH.
231
For example, pure water is in a chemical equilibrium.
232
There is exactly one hydronium ion for every 10 million water molecules.
233
In other words, the concentration of hydronium is 1 over 10 million, or 1 times 10 to the negative 7.
234
Taking the negative log of this gives us a pH of 7, which is considered neutral.
235
Anything lower than 7 is acidic, and anything above is basic, unlike you.
236
You can do the same thing with hydroxide ions and you will get the pOH, which keeps track of basicity.
237
Fun fact, the pH and pOH will always add up to 14 because they counteract each other, so by knowing one, you know both.
238
Now, if you have a strong base and a strong acid and you pour them together, no, they will not explode.
239
They will neutralize by forming water along with the salt, which is neutral.
240
For example, hydrochloride and sodium hydroxide will form water and table salt.
241
Oh yeah, speaking of table salt, remember how it consists of ionic bonds because sodium transfers an electron to chlorine,
242
well that is called a reduction oxidation reaction or redox.
243
If sodium chloride forms out of its pure elements, the sodium gets oxidized as it loses an electron,
244
and the chlorine gets reduced as it gains an electron.
245
Logically, sodium is the oxidant, and chlorine is the reductant.
246
Of course not, that would make sense, it's the other way around.
247
More accurately, redox reactions are reactions that change the oxidation numbers of elements, which are kind of like imaginary charges.
248
There's just a few rules you have to know to figure those out.
249
Hydrogen is mostly plus one.
250
Oxygen is mostly negative two.
251
Halogens are mostly negative one single elements are always zero
252
and the number of all atoms in a molecule always have to add up to the molecules charge.
253
So this would total zero while single ions just have their charge as the oxidation number.
254
For example in sulfuric acid we have four oxygens which totals negative eight, we have two hydrogens which brings the total to negative six,
255
and since the whole molecule is neutral sulfur must have an oxidation number of plus six.
256
Just by looking at the oxidation numbers of reactants
257
and products you can deduce the flow of electrons which gives you these equations.
258
If redox reactions happen in acidic or basic solutions, you can balance out the charges with ions and fix the stoichiometry with water.
259
Okay, now to this weird -looking thing.
260
I spared you from it because for describing electrons, this is very simple and this is not.
261
But this is actually like pretty wrong.
262
Electrons don't orbit in circles.
263
Here's how it actually works.
264
All electrons inside an atom are described by four quantum numbers.
265
N, L, ML, and MS. N corresponds to the shells, so all electrons with the same N are in the same shell.
266
Within the shells, we have subshells with multiple orbitals, which are three -dimensional regions in space where electrons could be.
267
We know these exist thanks to Schrodinger's equation, which gives a probabilistic wave function.
268
You can imagine it as a cloud, and the denser it is,
269
the more likely an electron is to be there if we were to look for it.
270
L describes the shape, and ML the orientation of orbitals in a subshell.
271
There are four subshells called S, P, D, and F.
272
If electrons have the same L, they're in the same subshell.
273
If electrons have the same N, L, and ML, they're in the same orbital.
274
Also, the number of orbitals increases by 2 for every bigger subshell, starting at just 1 for S.
275
The last quantum number describes an intrinsic property of electrons called spin, which can have two values.
276
Some guy named Pauli said two electrons can never have the exact same quantum numbers inside one atom.
277
Since MS can only have two values, every orbital defined by N, L, and ML can hold a maximum of two electrons with opposite spin.
278
Therefore, the S subshell can hold two electrons, the P subshell can hold 6, D can hold 10, and F can hold 14.
279
Now, the quantum numbers restrain each other like this, which means that the first shell can only have an S subshell,
280
the second can have an S and a P subshell, and so on.
281
This means that the first shell can hold a total of two electrons, the second can hold eight, the third can hold eighteen,
282
and generally the number of electrons a shell can hold follows the rule 2n squared, with n being the principal quantum number.
283
The principal quantum number, and therefore the total number of shells, increases from top to bottom in the periodic table, from one to seven.
284
Every element has a different number of electrons that fill up these orbitals,
285
and the different subshells and orbitals are filled in a specific order called the Aufbau Principle.
286
Just write down the subshells like this, and draw diagonal lines from top right to bottom left.
287
To get an electron configuration,
288
just look up the number of electrons of the element in the periodic table and fill up the subshells in this order,
289
until there are no electrons left.
290
This would be the electron configuration of sodium.
291
You can also look up the next smallest noble gas
292
and shorten it by just referring to its electron configuration as the base
293
because those shells are full and don't change for any bigger elements.
294
This is also how you can figure out the valence electrons for transition metals.
295
Just look up their electron configuration, ignore the full shells of the next smallest noble gas, and the remaining electrons are the valence electrons.
296
Easy peasy.
297
Anyways, all this knowledge is going to cost you one subscribe and a thumbs up, thank you very much.
298
Your comment is my delight and I shall now guide you, fine person, to the exit where the next lesson is excitedly waiting for you.
Uygulamayı İndir
Akıcı konuşmak için ihtiyacınız olan her şey
AI TelaffuzHer cümleyi puanla
IPA AlıştırmasıHer sesi ustalaştır
Kelime BilgisiKelime bankanızı oluşturun
Kelime OyunuOynarken öğrenin
FOR YOU
Video Öner
C12
35 cümleler
How Do Atoms Bond | Properties of Matter | Chemistry | FuseSchool
Daily ConversationUniversity Students
C11
339 cümleler
Introduction to HPLC - Lecture 1: HPLC Basics
Daily ConversationUniversity Students
C13
279 cümleler
LET THERE BE... Voltage? | Maxwell's Equation #2 Explained for Beginners
Daily ConversationUniversity Students
C11
167 cümleler
BLOOD TYPES explained in 9 Minutes
Daily ConversationUniversity StudentsWorking Adults
C12
474 cümleler
Metabolism | Electron Transport Chain: DETAILED | Part 1
Daily ConversationUniversity Students
C11
32 cümleler
Structure and Function of a Prokaryotic Cell (Bacteria)
Daily ConversationUniversity Students
C12
81 cümleler
What are substances made of ? | Lesson 5: MOLECULES—SIMPLE SUBSTANCES&COMPOUNDS | Science in English
Daily ConversationUniversity Students
C11
193 cümleler
Semiconductors explained in 16 mins | Chris Miller
Daily ConversationUniversity StudentsWorking Adults
C16
32 cümleler
What if quantum physics could eradicate illness? | Jim Al-Khalili for Big Think
Daily ConversationUniversity StudentsWorking Adults
B22
168 cümleler
The Truth About Nuclear Energy
Daily ConversationUniversity StudentsWorking Adults
B21
132 cümleler
Video
Daily ConversationUniversity StudentsWorking Adults
B25
49 cümleler
27 Facts That Will Make You Question Your Existence
Daily ConversationUniversity StudentsWorking Adults
Bu dersin kelimeleri ve konuşma notları
Bu konuşma dersi “GENERAL CHEMISTRY explained in 19 Minutes” videosuna dayanıyor. En çok tekrarlanan kelimeler: electron, reaction, element, energy, atom. Bu videoda gölgeleme çalışması için 64 cümle ve 4064 kelime var. Konuşma bölümü 18:49 sürüyor. Konuşmacı hızlı konuşuyor, dakikada yaklaşık 216 kelime; bu yüzden birbirine bağlanan ve zayıflayan sesler duyacaksınız. Kelimelerin yalnızca %77’i İngilizcede en sık kullanılan 3.000 kelime arasında, bu yüzden kelime dağarcığı zorlayıcı.
Bu videodaki önemli kelimeler
Videodan öğrenmeye değer 15 kelime, telaffuzu ve anlamıyla:
| Kelime | Telaffuz | Anlam |
|---|---|---|
| atom isim | /ˈætəm/ | atom |
| molecule isim | /ˈmɑ.lɪ.kjul/ | molekül |
| electron isim | /ɪˈlɛk.tɹɑn/ | elektron |
| shell isim | /ʃɛl/ | kabuk |
| hydrogen isim | /ˈhaɪdɹəd͡ʒ(ə)n/ | hidrojen, müvellidülmâ |
| element isim | /ˈɛləmənt/ | öğe, eleman |
| particle isim | /ˈpɑɹtək(ə)l/ | parçacık |
| ion isim | /ˈaɪ.ɑn/ | iyon |
| sodium isim | /ˈsəʊ.di.əm/ | sodyum |
| acid isim | /ˈæsɪd/ | asit |
| oxygen isim | /ˈɑksɪd͡ʒən/ | oksijen, müvellidülhumuza |
| substance isim | /ˈsʌbstəns/ | madde |
| quantum isim | /ˈkwɑntəm/ | kuantum, nicem |
| concentration isim | /ˌkɑn.sənˈtɹeɪ.ʃən/ | konsantrasyon, motivasyon |
| noble sıfat | /ˈnoʊbəl/ | soylu, asil |
Duyacağınız deyimsel fiiller
| Kelime | Telaffuz | Anlam |
|---|---|---|
| look up fiil | /ˌlʊk ˈʌp/ | yukarı bakmak |
| fall apart fiil | altüst olmak | |
| figure out fiil | açığa çıkarmak | |
| give off fiil | /ɡɪv ɒf/ | yaymak, saçmak |
| put together fiil | birleştirmek, bir araya getirmek | |
| throw away fiil | atmak |
Bu videodaki dil bilgisi
Konuşmacının en çok kullandığı yapılar, videodaki sözcüklerin aynısıyla:
| Yapı | Videoda |
|---|---|
| Koşul cümleleri if + cümle, will/would + fiil — bir koşul ve sonucu | if you give it enough energy, it will · If it's below zero, the water will spontaneously |
| Edilgen yapı be + fiilin üçüncü hâli — kimin yaptığı değil, ne olduğu önemli | is made · are called · is listed |
| İlgi cümlecikleri who / which + cümle — bir kişi ya da şey hakkında ek bilgi | core, which is · mass, which is · metals, which are |
Dikkat edilecek telaffuzlar
Konuşmacı don't, they're, doesn't gibi kısaltılmış biçimleri 28 kez kullanıyor. Bunları duyduğunuz gibi kısa söyleyin.
- “th” sesleri: thumb /ˈθʌm/, endothermic /ˌɛndəʊˈθəːmɪk/, enthalpy /ˈɛn.θəl.piː/
- “sh” ve “zh” sesleri: shell /ʃɛl/, concentration /ˌkɑn.sənˈtɹeɪ.ʃən/, equation /ɪˈkweɪ.ʒən/, configuration /kənˌfɪɡ.əˈɹeɪ̯.ʃən/, transition /tɹænˈzɪʃ.ən/
- Uzun kelimeler — vurguyu doğru yere koyun: periodic /ˌpɪɹiˈɑdɪk/, concentration /ˌkɑn.sənˈtɹeɪ.ʃən/, configuration /kənˌfɪɡ.əˈɹeɪ̯.ʃən/, spontaneous /spɑnˈteɪ.ni.əs/, equilibrium /ɛkwɪˈlɪbɹɪəm/
Türkçe konuşanların zorlandığı sesler:
- /w/ — dudaklar yuvarlak, /v/ değil: quantum /ˈkwɑntəm/, equation /ɪˈkweɪ.ʒən/, equilibrium /ɛkwɪˈlɪbɹɪəm/, liquid /ˈlɪk.wɪd/, whereas /(h)wɛɹˈæz/
- Kelime başındaki ünsüz kümesi — araya ünlü eklemeyin: quantum /ˈkwɑntəm/, gram /ˈɡɹæm/, spontaneous /spɑnˈteɪ.ni.əs/, grid /ɡɹɪd/, freely /ˈfɹili/
- /æ/ — “e”den daha açık: atom /ˈætəm/, acid /ˈæsɪd/, react /ɹiːˈækt/, gram /ˈɡɹæm/, transition /tɹænˈzɪʃ.ən/
Bu videoyla nasıl çalışılır
- Videonun tamamını konuşmadan bir kez dinleyin ve bilmediğiniz kelimeleri not edin.
- 0,75× hızla başlayın, cümle cümle tekrar edin ve kolaylaşınca normal hıza dönün.
- Kendinizi kaydedin ve orijinaliyle karşılaştırın; atom, molecule, electron gibi kelimelere özellikle dikkat edin.
Gölgeleme Tekniği Nedir?
Gölgeleme, başlangıçta profesyonel tercüman eğitimi için geliştirilen ve çok dilli Dr. Alexander Arguelles tarafından popüler hale getirilen, bilim destekli bir dil öğrenme tekniğidir. Yöntem basit ama güçlüdür: ana dili İngilizce olan bir sesi dinler ve hemen yüksek sesle tekrar edersiniz — konuşmacıyı 1-2 saniye gecikmeyle takip eden bir gölge gibi. Pasif dinleme veya dilbilgisi alıştırmalarının aksine, gölgeleme beyninizi ve ağız kaslarınızı gerçek konuşma kalıplarını eşzamanlı olarak işlemeye ve yeniden üretmeye zorlar. Araştırmalar, telaffuz doğruluğu, tonlama, ritim, bağlı konuşma, dinleme anlama ve konuşma akıcılığını önemli ölçüde geliştirdiğini göstermektedir — bu da onu IELTS Konuşma hazırlığı ve gerçek dünya İngilizce iletişimi için en etkili yöntemlerden biri yapar.