쉐도잉 연습: GENERAL CHEMISTRY explained in 19 Minutes - 영상으로 영어 말하기 배우기

연습 모드 선택

각 모드는 전체 화면 연습실로 열립니다.

298 문장

문장이 너무 짧거나 길면 Edit를 눌러 조정하세요.

Everything is made of atoms.

Yes, even you.

Atoms consist of a core and some electrons.

The core is made of protons and neutrons, and depending on the number of protons, you get different elements.

Water is made of hydrogen and oxygen.

This is some sodium.

Hmm, I wonder what happens when you...

Ha, whoopsie.

Quantum mechanics tells us that this is not what atoms actually look like.

They look more like this, but we'll get to that later.

For now, just think of atoms as having multiple electron shells.

The electrons in the outermost shell are called valence electrons.

Most of chemistry is really just the behavior of these electrons.

Every element is listed in the periodic table.

All elements in the same column or group have the same number of valence electrons.

For the main groups, the number of valence electrons is just the group number from 1 to 8.

Except for helium.

It's too small to have 8 electrons, it can only have 2, but still, it acts like a noble gas,

so it's just kinda grouped in with those.

Luckily, the transition metals also follow a nice pattern.

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.

Elements with the same number of valence electrons tend to show similar behavior in chemical reactions.

For example, the first group without hydrogen is called the alkali metals.

Here's some things they have in common.

They have one valence electron, they're shiny metals, they're kind of soft, and they do this sometimes.

All elements in the same row or period have the same number of shells.

This number increases from top to bottom.

Also, the mass gets bigger from left to right, as each element gains a proton, an electron, and some neutrons.

Depending on the number of neutrons in the core, you get different isotopes of the same element,

most of which are pretty unstable and fall apart, releasing ionizing radiation.

Fun fact, that stuff will kill you.

If an atom has the same amount of electrons as protons, it has no charge.

If it has more, it has a negative charge, and if it has less, it has a positive charge.

Charged atoms are called ions.

Negative ions are anions, and positive ions are cations.

The periodic table is also pretty much a dictionary, as every cell tells you the name and symbol of an element,

the number of protons in the core, which is also the total number of electrons,

and the atomic mass, which is the mass of neutrons and protons combined.

The periodic table is roughly divided into three categories.

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,

which have properties that fall somewhere in between.

Two or more atoms bonded together form a molecule.

If you have at least two different elements, you get a compound.

Oh yeah, this is probably a good time to mention that compounds often behave completely differently than the elements they're made of.

Like you put together an explosive metal and a toxic gas, and you get, of course, an even more expli - Table salt.

You get table salt.

There's many ways to write molecules, for example the molecular formula, where you just count the number of each atom in a molecule

and write them as a subscript number next to the element symbol.

But that has some problems, look at these two molecules.

They have the same molecular formula, but obviously they're not the same.

They're isomers.

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,

and I don't think anyone's gonna go, well, yes, this dusty black blob is indeed very expensive.

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.

This is also going to help us understand why atoms bond in the first place.

You see, everything in the universe wants to get to a state of lower energy.

That's why a ball on a hill will roll down by itself, because that decreases its potential energy.

This trend also applies to atoms.

The state of lowest potential energy is having a full outer shell of electrons, which is most often eight,

or in the case of hydrogen and helium, too.

If you think back to the periodic table, you'll see that all noble gases already have a full outer shell,

which is why they don't really want to react with anything.

If two atoms don't have a full outer shell, but can achieve one by sharing electrons, they will naturally do so,

the same way a ball will go downhill, as their combined energy would be lower than if they were separate.

The sharing of electrons is called a covalent bond.

These bonds are also caused by the positively charged nucleus of an atom tugging on electrons of another atom.

The strength of this pole is called electronegativity.

In the periodic table, the electronegativity increases from bottom left to the top right.

Therefore, fluorine has the strongest pull.

It's just unbelievably desperate for an electron.

If the difference in electronegativity is bigger than about 1 .7, you get an ionic bond.

A good example is sodium chloride.

Chlorine would do anything for an electron, while sodium has one too many and just kinda wants to get rid of it anyway.

Perfect, they both say, forming an ionic bond, where sodium loses an electron and turns into a cation,

and chlorine gains an electron and turns into an anion.

That seems pretty important.

You might want to remember it.

The most common place you see ionic bonds is in salt.

Yes, also table salt, but more generally when metals and non -metals bond you get a salt, which is just a grid of ions.

Speaking of metals, a pure metal forms metallic bonds.

You can imagine this as a huge grid of positively charged nuclei, which are surrounded by freely moving electrons.

You see, in a metal grid, the valence electrons are kinda promiscuous, or as the nerds call it, delocalized.

They can move freely in a giant playground of nuclei instead of being loyal to just one.

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.

Like, you can hammer on this stuff until it's the most deformed, unelegant, and ugly -looking piece of material ever known,

and it will just limp along as if nothing ever happened.

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.

If it's bigger than 0 .5 but smaller than around 1 .7, one of the elements is pulling on the electrons pretty hard.

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.

An example is water.

Oxygen has a very high electronegativity compared to hydrogen.

As a result, it pulls the electrons of hydrogen so hard that they kind of belong to oxygen, giving it a partial negative charge,

and leaving hydrogen with a partial positive charge.

The presence of two poles with opposite charge is called an electric dipole.

All permanent dipole molecules can interact with each other, and really with anything that has a charge.

As a result, the molecules will tug on each other

and arrange themselves in a way that oppositely charged ends are next to each other.

The forces acting between them are called intermolecular forces, or IMFs.

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.

앱 다운로드

유창하게 말하는 데 필요한 모든 것

AI 발음 평가문장마다 점수 확인

IPA 발음 연습모든 소리 마스터

단어 학습나만의 단어장 만들기

단어 게임놀면서 외우기

QR 스캔

Download on theApp Store Get it onGoogle Play

FOR YOU

이 레슨의 어휘와 말하기 포인트

이 말하기 레슨은 영상 “GENERAL CHEMISTRY explained in 19 Minutes”을(를) 바탕으로 합니다. 가장 자주 반복되는 단어는 다음과 같습니다: electron, reaction, element, energy, atom. 이 영상에는 섀도잉할 문장 64개와 단어 4064개가 있습니다. 말하는 구간의 길이는 18:49입니다. 화자는 분당 약 216단어로 빠르게 말하므로 연음과 약하게 발음되는 소리가 많습니다. 영어에서 가장 많이 쓰이는 3,000단어에 속하는 단어가 77%뿐이라 어휘가 어려운 편입니다.

이 영상의 핵심 어휘

영상에 나오는 익혀 둘 만한 단어 15개를 발음, 뜻과 함께 정리했습니다.

단어	발음	뜻
atom 명사	/ˈætəm/	원자, 아톰
molecule 명사	/ˈmɑ.lɪ.kjul/	분자
electron 명사	/ɪˈlɛk.tɹɑn/	전자
shell 명사	/ʃɛl/	조가비, 조개
hydrogen 명사	/ˈhaɪdɹəd͡ʒ(ə)n/	수소
element 명사	/ˈɛləmənt/	요소
particle 명사	/ˈpɑɹtək(ə)l/	입자, 립자
ion 명사	/ˈaɪ.ɑn/	이온
sodium 명사	/ˈsəʊ.di.əm/	나트륨, 소듐
acid 명사	/ˈæsɪd/	산
oxygen 명사	/ˈɑksɪd͡ʒən/	산소
substance 명사	/ˈsʌbstəns/	물질
concentration 명사	/ˌkɑn.sənˈtɹeɪ.ʃən/	집중, 집중력
react 동사	/ɹiːˈækt/	반응하다
equation 명사	/ɪˈkweɪ.ʒən/	방정식

영상에 나오는 구동사

단어	뜻
put together 동사	조립하다
throw away 동사	버리다
write down 동사	적다, 적어 두다

이 영상의 문법

화자가 가장 많이 쓰는 문형을 영상 속 실제 표현과 함께 정리했습니다.

문형	영상 속 표현
조건문 if + 절, will/would + 동사 — 조건과 그 결과	if you give it enough energy, it will · If it's below zero, the water will spontaneously
수동태 be + 과거분사 — 누가 하는지보다 무슨 일이 일어나는지에 초점	is made · are called · is listed
관계절 who / which + 절 — 사람이나 사물에 대한 추가 정보	core, which is · mass, which is · metals, which are

주의할 발음

화자는 don't, they're, doesn't 같은 축약형과 약화된 형태를 28번 사용합니다. 들리는 대로 짧게 발음하세요.

“th” 소리: thumb /ˈθʌm/, endothermic /ˌɛndəʊˈθəːmɪk/, enthalpy /ˈɛn.θəl.piː/
“sh”와 “zh” 소리: shell /ʃɛl/, concentration /ˌkɑn.sənˈtɹeɪ.ʃən/, equation /ɪˈkweɪ.ʒən/, configuration /kənˌfɪɡ.əˈɹeɪ̯.ʃən/, transition /tɹænˈzɪʃ.ən/
긴 단어 — 강세 위치에 주의: periodic /ˌpɪɹiˈɑdɪk/, concentration /ˌkɑn.sənˈtɹeɪ.ʃən/, configuration /kənˌfɪɡ.əˈɹeɪ̯.ʃən/, spontaneous /spɑnˈteɪ.ni.əs/, equilibrium /ɛkwɪˈlɪbɹɪəm/

한국어 화자가 어려워하는 소리:

/f/ — ㅍ(/p/)으로 바꾸지 말고 윗니를 아랫입술에 대기: configuration /kənˌfɪɡ.əˈɹeɪ̯.ʃən/, freely /ˈfɹili/, formula /ˈfɔː.mjʊ.lə/, refer /ɹɪˈfɜː/, frequency /ˈfɹiːkwənsi/
/v/ — ㅂ(/b/)과 구별하기: divide /dɪˈvaɪd/, positively /ˈpɑ.zɪ.tɪv.li/, activation /ˌæktəˈveɪʃən/, evenly /ˈiːvənli/, conservation /ˌkɑnsə(ɹ)ˈveɪʃən/
/z/ — ㅈ이 아니라 성대를 울리는 /s/: transition /tɹænˈzɪʃ.ən/, positively /ˈpɑ.zɪ.tɪv.li/, whereas /(h)wɛɹˈæz/, exit /ˈɛɡzət/, freeze /ˈfɹiːz/

이 영상으로 연습하는 방법

먼저 말하지 않고 영상을 끝까지 듣고 모르는 단어를 적어 둡니다.
0.75배속으로 한 문장씩 섀도잉을 시작하고, 익숙해지면 보통 속도로 돌아갑니다.
자신의 목소리를 녹음해 원본과 비교하고, atom, molecule, electron 같은 단어에 특히 주의합니다.

쉐도잉이란? 영어 실력을 빠르게 키우는 과학적 방법

쉐도잉(Shadowing)은 원래 전문 통역사 훈련을 위해 개발된 언어 학습 기법으로, 다언어 학자인 Dr. Alexander Arguelles에 의해 대중화된 방법입니다. 핵심 원리는 간단하지만 매우 강력합니다: 원어민의 영어를 들으면서 1~2초의 짧은 지연으로 즉시 소리 내어 따라 말하는 것——마치 '그림자(shadow)'처럼 화자를 따라가는 것입니다. 문법 공부나 수동적인 청취와 달리, 쉐도잉은 뇌와 입 근육이 동시에 실시간으로 영어를 처리하고 재현하도록 훈련합니다. 연구에 따르면 이 방법은 발음 정확도, 억양, 리듬, 연음, 청취력, 말하기 유창성을 크게 향상시킵니다. IELTS 스피킹 준비와 자연스러운 영어 소통을 원하는 분들에게 특히 효과적입니다.

섀도잉 방법: 단계별 전체 가이드 읽기 →

쉐도잉 연습: GENERAL CHEMISTRY explained in 19 Minutes - 영상으로 영어 말하기 배우기

연습 모드 선택

앱 다운로드

추천 영상

How Do Atoms Bond | Properties of Matter | Chemistry | FuseSchool

Introduction to HPLC - Lecture 1: HPLC Basics

LET THERE BE... Voltage? | Maxwell's Equation #2 Explained for Beginners

BLOOD TYPES explained in 9 Minutes

Metabolism | Electron Transport Chain: DETAILED | Part 1

Structure and Function of a Prokaryotic Cell (Bacteria)

What are substances made of ? | Lesson 5: MOLECULES—SIMPLE SUBSTANCES&COMPOUNDS | Science in English

Semiconductors explained in 16 mins | Chris Miller

What if quantum physics could eradicate illness? | Jim Al-Khalili for Big Think

The Truth About Nuclear Energy

Video

27 Facts That Will Make You Question Your Existence