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82. 10-МАРАФОН ОРГАНИЧЕСКИХ ЦЕПОЧЕК

82. 10-МАРАФОН ОРГАНИЧЕСКИХ ЦЕПОЧЕК

Channel: Птичка Химичка -Химия с Нуля-

18. Циклоалканы (часть 2)

18. Циклоалканы (часть 2)

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38. Водород. Химические свойства

38. Водород. Химические свойства

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43. Соли. Классификация

43. Соли. Классификация

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30. Количество вещества. Тест (часть 4)

30. Количество вещества. Тест (часть 4)

Channel: Птичка Химичка -Химия с Нуля-

64. Степени окисления элементов (часть 2)

64. Степени окисления элементов (часть 2)

Channel: Птичка Химичка -Химия с Нуля-

54. Электронное строение атома (часть 3)

54. Электронное строение атома (часть 3)

Channel: Птичка Химичка -Химия с Нуля-

59. Определяем тип химической связи в веществе

59. Определяем тип химической связи в веществе

Channel: Птичка Химичка -Химия с Нуля-

61. Аминокислоты (часть 1)

61. Аминокислоты (часть 1)

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77. 7-МАРАФОН ОРГАНИЧЕСКИХ ЦЕПОЧЕК

77. 7-МАРАФОН ОРГАНИЧЕСКИХ ЦЕПОЧЕК

Channel: Птичка Химичка -Химия с Нуля-

химия с нуля

егэ по химии

огэ по химии

химия на отлично

школьная химия

химическая связь

типы химических связей

атомная кристаллическая решетка

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электроотрицательность

химияснуля,

егэхимия,

огэхимия,

химиянаотлично,

химическаясвязь,

типыхимическихсвязей,

атомнаякристаллическаярешетка,

молекулярнаякристаллическаярешетка,

ковалентнаясвязь,

ковалентнаяполярнаясвязь,

ковалентнаянеполярнаясвязь,

00:00:00

hello, we are continuing the topic of chemical

00:00:03

bonding and today we will look in detail at

00:00:05

how a covalent bond is formed and in

00:00:08

what compounds it is realized. To

00:00:11

understand how a covalent bond is formed,

00:00:13

we will again have to remember the

00:00:15

electronic structure of an atom, because everything that

00:00:18

happens to atoms is directly related to the

00:00:21

structure of their external energy

00:00:23

level, well and of course, as an

00:00:26

example, let’s consider a compound as much as chlorine; in

00:00:29

this compound, a covalent bond will be realized;

00:00:33

what is it like? To

00:00:36

understand this, let’s remember what the external

00:00:38

and electronic levels in a hydrogen and

00:00:42

chlorine atom look like; a hydrogen atom contains only

00:00:45

one electron and it is naturally located

00:00:49

on one from the sublevels, that is, the first

00:00:51

level is already the

00:00:53

outer layer of chlorine for hydrogen, only 17 electrons

00:00:57

of which 7 are located on the outer third

00:00:59

level, if we look carefully we

00:01:02

will see that hydrogen has a single

00:01:04

electron and it is, of course, unpaired, and the

00:01:07

chlorine atom has 7 electrons on the outer level

00:01:09

of which 6 form three

00:01:12

pairs, one electron remains without a pair,

00:01:15

it is unpaired and we write graphically the

00:01:18

electronic formulas for these atoms:

00:01:21

one unpaired electron in hydrogen and

00:01:23

one unpaired electron in chlorine,

00:01:26

the remaining six electrons on the outer

00:01:28

level form three pairs, how

00:01:31

will a covalent

00:01:34

bond be formed? We can see that before the completion of the

00:01:39

outer level, the hydrogen atom

00:01:42

lacks one electron, because the 1c sub

00:01:45

level can contain a maximum of two

00:01:47

electrons,

00:01:48

and the first level consists of only 1c sub

00:01:51

level, so for the first level to be

00:01:53

completely filled, hydrogen must have

00:01:56

two electrons 1, that is,

00:01:58

one hydrogen electron is missing

00:02:01

Chlorine has 7 electrons on the outer level and

00:02:04

for it to be completely filled,

00:02:07

one electron is also missing, if you

00:02:09

add one more electron here it will be 8

00:02:11

electrons,

00:02:12

and what happens between these

00:02:15

atoms, a common electron pair is formed between them,

00:02:20

that is, each of the atoms provides for

00:02:23

common use its unpaired

00:02:25

electron and, most importantly, this common

00:02:29

electron pair

00:02:30

simultaneously belongs to both atoms, that

00:02:34

is, it is a pair of electrons for the

00:02:37

hydrogen atom and it is also a pair of

00:02:40

electrons for the chlorine atom, so it

00:02:43

turns out that the hydrogen atom now has

00:02:46

two electrons and this is a completely

00:02:48

filled outer level 1 that is, the

00:02:52

hydrogen atom acquired a stable

00:02:54

electronic configuration of the noble gas

00:02:57

helium, and the chlorine atom now has 8

00:03:01

electrons; it had seven and another one

00:03:04

it took for use from the hydrogen atom;

00:03:06

now it has a total of 8 electrons, and

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this is also the stable electronic

00:03:12

configuration of the noble inert gas,

00:03:14

that is, now the level of each atom is

00:03:17

completely filled with electrons, it is in

00:03:20

this state that the atoms are most active,

00:03:23

so we remember that a covalent bond

00:03:26

is always the formation of common electron

00:03:29

pairs, a common electron pair belongs

00:03:33

simultaneously to all the ataman who

00:03:35

participated in their formation; in fact,

00:03:39

one electron pair is one

00:03:42

covalent bond, an

00:03:43

electron pair in graphic in formulas

00:03:46

they are represented by a dash, now we

00:03:48

remember that a dash

00:03:50

means one common electron

00:03:52

pair, and as an example, consider the

00:03:56

nitrogen molecule nitrogen molecules consists of

00:04:00

two hydrogen and nitrogen atoms, of course

00:04:04

we remember substances simple non-metals of

00:04:08

molecular structure h2 n 2 o 2 fluorine 2

00:04:12

chlorine 2 Bruce

00:04:13

together 2 why do these substances not

00:04:15

exist in the form of individual atoms, but

00:04:18

form diatomic molecules? Again,

00:04:21

this is due to the structure of their external

00:04:24

energy level. Let’s consider what

00:04:28

it looks like for a nitrogen atom; nitrogen at the

00:04:31

external level has 5 electrons, since nitrogen

00:04:34

is in group 5; all these

00:04:37

we should already know the rules and patterns,

00:04:39

and of these 5 electrons, 2 form a

00:04:43

pair on 2s sublevels and three are

00:04:46

unpaired,

00:04:48

and accordingly, the second

00:04:49

nitrogen atom will have the same situation if we

00:04:52

draw graphic

00:04:55

electronic formulas for nitrogen atoms, we

00:04:58

can distribute the electrons in this

00:04:59

way, here’s one a pair of electrons two from

00:05:02

under the level and and contains 3 unpaired

00:05:05

electrons since each nitrogen atom has

00:05:08

only 5 electrons and it is obvious that before

00:05:10

the level is completed, each nitrogen atom

00:05:13

lacks 3 electrons, which means somewhere these

00:05:16

three electrons need to be taken and that’s how

00:05:19

each of the atoms nitrogen borrows these

00:05:22

three electrons from a neighboring atom and what we

00:05:25

get as a result is that between two

00:05:27

nitrogen atoms,

00:05:30

common electron pairs are simultaneously formed from perry and 1 2 and 3,

00:05:36

respectively, all three electron pairs

00:05:39

belong to the first nitrogen atom and

00:05:41

now it has 8 electrons in total and the

00:05:44

second nitrogen atom and it also has

00:05:47

a total of 8 electrons, that is, the external

00:05:50

levels of these atoms are completely filled, which

00:05:53

means they are stable, and of course, since

00:05:56

one electron pair is one

00:05:58

covalent bond,

00:05:59

one dash, then between two

00:06:02

nitrogen atoms we will draw three dashes because

00:06:05

three common electrons have been formed

00:06:07

pairs and this means that in a nitrogen molecule

00:06:10

between two nitrogen atoms there are 3

00:06:14

covalent bonds,

00:06:15

remember that a covalent bond is equal to the total

00:06:18

electron pair, the number of electron pairs

00:06:21

indicates the number of the bond,

00:06:23

everything is very simple, I think that here you

00:06:26

just need to remember what an electron

00:06:29

pair is and how it is designated in

00:06:31

graphical formulas, we will look at

00:06:33

another example, a water molecule, what kind of bonds

00:06:37

are formed here, again for this we

00:06:40

need to remember what the outer energy level looks like

00:06:44

in an oxygen atom on the

00:06:47

outer level oxygen has 6 electrons,

00:06:49

4 of them form two pairs

00:06:53

and two electrons remain unpaired and

00:06:56

we In this way we denote two pairs of

00:06:58

electrons and two unpaired electrons, a

00:07:01

total of 6 electrons at the outer level,

00:07:03

and each hydrogen atom, of course, has

00:07:07

one unpaired electron; oxygen

00:07:09

lacks two electrons to complete

00:07:11

the level,

00:07:12

and each hydrogen lacks one

00:07:15

electron, so two hydrogens per

00:07:18

atom oxygen form

00:07:20

common electron pairs and we remember that a

00:07:24

common electron pair

00:07:25

is called common because it simultaneously

00:07:27

belongs to one atom

00:07:29

and in the second case, a water molecule, oxygen

00:07:33

formed two common pairs with two

00:07:36

hydrogen atoms, now oxygen has a total of 8

00:07:39

electrons on the outer level and each

00:07:42

hydrogen has formed one electron

00:07:44

and a

00:07:45

common electron pair with an

00:07:47

oxygen atom, and now each hydrogen has

00:07:49

two electrons on the outer level and also the

00:07:52

outer level is the first and only one in the

00:07:56

hydrogen atom is filled completely in

00:07:59

this state, of course the atoms will be

00:08:01

stable, so the covalent bond is

00:08:03

quite strong, these are the common

00:08:06

electron pairs they are

00:08:08

atoms are very firmly connected to each other,

00:08:10

and how does this

00:08:12

bonding occur

00:08:13

and what, in principle, is a

00:08:16

covalent bond? the nucleus of the oxygen atom is

00:08:20

naturally charged positively like

00:08:23

all the nuclei of all other atoms,

00:08:25

so the positive oxygen nucleus

00:08:28

will attract negative

00:08:30

electrons of hydrogen due to this

00:08:34

its own image,

00:08:35

this is an electron pair, these

00:08:37

hydrogen electrons are attracted by the oxygen nucleus,

00:08:40

and the hydrogen nuclei attract

00:08:44

oxygen electrons, that is, it turns out that these

00:08:47

electron shells seem to penetrate

00:08:50

one another precisely due to the

00:08:53

attraction of the electrons of the neighboring

00:08:56

poison atom and the atomic nuclei,

00:08:59

that is, you need to clearly understand what is a

00:09:02

covalent bond? This is a type of

00:09:05

electrostatic interaction in

00:09:08

which the nucleus of one atom

00:09:11

attracts the electrons of another atom. And

00:09:13

of course, if we graphically depict a

00:09:15

water molecule, we understand that we have

00:09:17

formed two common electron pairs and

00:09:20

one each between two hydrogen and

00:09:25

oxygen atoms, which means 2 covalent bonds depart from oxygen,

00:09:28

and oxygen

00:09:30

formed two pairs,

00:09:33

one covalent bond departs from each hydrogen, and

00:09:36

each hydrogen

00:09:37

participates in the formation of only one

00:09:39

common electron pair. Well, let’s remember

00:09:43

what a covalent bond is, this is an

00:09:46

electrostatic interaction, we remember

00:09:48

what electrostatic

00:09:50

interactions are when plus attracts

00:09:51

minus, this is the electrostatic

00:09:54

interaction between the positive nucleus of

00:09:57

one atom and the negatively charged

00:10:00

electrons of another atom, this is a

00:10:03

covalent bond, the most important thing we

00:10:05

must remember is that a covalent bond

00:10:08

is always the formation of shared electron

00:10:11

pairs, the

00:10:12

number of bonds depends on the number of shared

00:10:15

electron pairs

00:10:16

if the pair is 1 pi -bond 1 if part 2 to and

00:10:20

bonds and two and so on the next thing we will

00:10:24

consider regarding the covalent bond is

00:10:26

also to find out in which compounds it

00:10:29

is realized, so the covalent bond

00:10:32

is realized only between

00:10:35

metal atoms if before we considered the

00:10:38

metallic bond and said that it

00:10:40

arises only between metal atoms

00:10:43

and identical metal atoms, that

00:10:46

is, a

00:10:48

metallic bond does not arise between all alme atoms, then a

00:10:51

covalent bond arises precisely

00:10:54

only between non-metal atoms, and

00:10:57

based on this, a covalent bond is also

00:11:01

further divided into polar

00:11:03

and non-polar, how can we distinguish them?

00:11:06

molecules consisting

00:11:08

only of non-metal atoms, of course,

00:11:11

this bond is covalent, there

00:11:14

will be no other way, but how to understand in which case it is

00:11:17

polar and in which case it is non-polar,

00:11:20

so a polar covalent bond

00:11:23

arises between atoms with different

00:11:26

electronegativity, they are polar

00:11:28

between atoms with the same, so what

00:11:32

electronegativity is something you need to

00:11:34

remember well because this is a

00:11:36

very important parameter characterizing

00:11:38

atoms electronegativity is the

00:11:41

ability of an atom to shift a common

00:11:45

electron pair towards itself, of course, the higher the

00:11:49

electronegativity values, the

00:11:51

stronger it is, and then it pulls over

00:11:54

this common pair of electrons, which

00:11:56

was formed as a result of the interaction of

00:11:59

atoms, well,

00:12:01

there are tables that

00:12:05

already indicate specific numerical values of

00:12:06

electronegativity, for example, here is a

00:12:09

table of electronegativity from

00:12:11

NGU where for each element of the main

00:12:14

subgroup the numerical value of

00:12:17

electronegativity is indicated, we can see

00:12:19

that fluorine has the highest

00:12:22

electronegativity equal to 4, which

00:12:24

means that fluorine

00:12:26

will always displace the electron

00:12:29

pair by No one

00:12:32

will ever be able to

00:12:34

take away this electron pair from fluorine because fluorine has the

00:12:36

highest electronegativity

00:12:38

and electronegativity is precisely the

00:12:40

ability of an atom to shift a

00:12:43

common electron pair towards itself, and if we

00:12:45

look carefully at this plate we

00:12:47

will see such a pattern in the periods

00:12:51

electronegativity will be

00:12:52

increase from left to right,

00:12:55

that is, when moving from metals to

00:12:57

metals, and we can draw such an important

00:13:00

conclusion that for mid

00:13:01

olaf the electronegativity will be

00:13:04

minimal and for her metals it will be

00:13:07

maximum in each period in groups

00:13:11

electronegativity increases

00:13:12

from bottom to top, that is, of all the halogens of the

00:13:17

elements of the seventh group of the main

00:13:19

subgroups, the highest

00:13:21

electronegativity will be for fluorine,

00:13:23

the lowest electronegativity

00:13:25

will be for as to the so even if

00:13:28

we don’t have a tablet indicating the

00:13:30

electronegativity values, we

00:13:33

can use the usual

00:13:34

periodic table, but we must

00:13:36

remember exactly this

00:13:38

pattern of how

00:13:40

electronegativity changes in periods and

00:13:42

groups and let’s look at an example: in

00:13:45

periods, electronegativity always

00:13:47

increases from left to right from metal to

00:13:51

metal, and in groups it always

00:13:53

increases from bottom to top, you need to

00:13:57

remember this important rule very well,

00:13:59

and now that we know what the

00:14:02

electronegativity of an atom is and how it

00:14:05

changes for different elements in a period

00:14:10

and in a group we can divide a

00:14:12

covalent bond into polar and non-

00:14:15

polar, for this we need to understand

00:14:18

that a polar covalent bond

00:14:22

is realized between non-metal atoms with

00:14:26

different electronegativity there is a

00:14:30

covalent bond it is always a bond between

00:14:32

non-metal atoms but these non-metals

00:14:35

can have the same electronegativity values but

00:14:39

they can have different ones, so if a bond

00:14:42

has arisen between non-metal atoms with

00:14:44

different electronegativity, it

00:14:46

will always be a covalent polar bond, why is it

00:14:49

called that, what

00:14:51

happens in a molecule when

00:14:53

such a bond is formed, let’s also consider an example

00:14:57

and, as an example, consider a molecule

00:14:58

as much as chlorine, we have already discussed in at the beginning that in the

00:15:01

chlorine molecule one common

00:15:04

electron pair is formed, well, we understand that the

00:15:07

bond is covalent because it

00:15:09

was formed between two

00:15:12

non-metallic atoms hydrogen is not a

00:15:14

metal and chlorine is not a metal one pair means

00:15:17

this is one covalent bond,

00:15:20

naturally it will be polar and because

00:15:23

and and formed this connection of 2

00:15:26

non-metallic elements with different

00:15:29

electronegativity me if we

00:15:31

look at the

00:15:32

electronegativity table we will see that the

00:15:34

electronegativity of chlorine is

00:15:37

greater than the electronegativity of

00:15:39

hydrogen and this means that chlorine will

00:15:41

shift the common electron pair towards itself,

00:15:45

that is, it will move it away from hydrogen

00:15:48

and how this pair will approach to the

00:15:52

chlorine atom,

00:15:53

what is happening here is the most important thing,

00:15:57

taking into account the fact that

00:16:01

one extra electron is moving towards the chlorine atom, which was initially neutral, this is a

00:16:04

hydrogen electron, even if it

00:16:06

was not initially in the chlorine, but now it has moved towards the chlorine

00:16:09

since the electron carries a

00:16:11

negative charge in the tones a

00:16:14

partial negative charge appears

00:16:17

and on hydrogen it is partial positive,

00:16:20

this is important to remember if a covalent

00:16:23

bond is formed by non-metal atoms with different

00:16:27

electronegativity, that pair of

00:16:29

electrons

00:16:30

in common always shifts to a more

00:16:34

electronegative atom and a

00:16:36

partial negative charge always appears on it,

00:16:39

and the atom from which the pair

00:16:42

has moved away receives a partial

00:16:44

positive charge, why are these charges

00:16:48

partial they are designated delta plus

00:16:50

and delta minus because the electron does not

00:16:53

completely transfer from hydrogen to chlorine,

00:16:56

it’s not that hydrogen gave up one minus and

00:16:59

became one plus, and chlorine took one

00:17:02

minus and became one minus

00:17:05

charge, chlorine got one minus, it’s not so

00:17:08

important to remember the

00:17:10

electron does not completely transfer to chlorine,

00:17:12

it still simultaneously belongs to its

00:17:15

hydrogen

00:17:16

and chlorine, all this pair belongs to its

00:17:18

people and chlorine, but taking into account the fact that all the

00:17:21

same electrons have moved to chlorine, then a

00:17:24

negative cloud appears on it, a

00:17:29

negative electron density

00:17:32

increases on the chlorine atoms and this is possible

00:17:35

consider the example of such

00:17:38

graphic images, that is, when in

00:17:40

one molecule, and this is still one

00:17:42

molecule, a

00:17:47

negative charge is formed on one pole and a

00:17:49

positive charge is concentrated on the other pole,

00:17:52

such a molecule is called a dipole, that

00:17:55

is, we have two poles, plus and minus,

00:17:57

and since these poles 2 hence

00:18:00

the name de

00:18:01

these are two fields from the word pole dipole and

00:18:05

so molecules

00:18:07

containing covalent polar bonds

00:18:10

are always dipoles

00:18:12

and you can see how the

00:18:14

electron density is distributed in

00:18:16

such a molecule we are told that the common

00:18:19

electron pair of the

00:18:21

opar is the electron density,

00:18:23

that is, the

00:18:24

concentration of electrons shifts to the

00:18:27

more electronegative chlorine, a

00:18:30

partial

00:18:33

negative charge appears on chlorine, and on hydrogen,

00:18:35

since electrons have moved away from it, a

00:18:37

partial positive charge arises, the

00:18:40

value of this charge is always greater than 0, well,

00:18:43

less than one, because if suddenly

00:18:45

the charge becomes equal to one, this means

00:18:48

that the electron has completely transferred from the

00:18:51

hydrogen atom This does not happen to the chlorine atom in covalent

00:18:54

polar compounds; the

00:18:57

electrons are not completely transferred but are

00:18:59

simply partially displaced, but at the same time the

00:19:02

electron pair still

00:19:05

belongs to both

00:19:06

hydrogen and their chlorine. I hope that

00:19:08

this is clear, that is, a covalent

00:19:11

polar bond always occurs between

00:19:14

different

00:19:17

non-metal atoms different precisely in

00:19:20

electronegativity, and examples in

00:19:23

which compounds a

00:19:26

covalent polar bond can be realized, firstly in

00:19:29

acidic oxides,

00:19:30

most oxides are a combination of

00:19:34

oxygen with non-metals,

00:19:36

and we know that a covalent bond is

00:19:39

just a bond between non-metals, for example co2

00:19:42

is an acid oxide,

00:19:44

carbon monoxide and carbon and oxygen

00:19:46

non-metals but 1 2 not metals means there is

00:19:49

definitely a covalent bond between them,

00:19:51

well since these non-metals are different it means there is a

00:19:53

covalent polar bond between them the same

00:19:56

thing in a water molecule in a molecule as much as chlorine

00:19:59

in an ammonia molecule and nitrogen and hydrogen

00:20:01

are not a metal and they are different in

00:20:04

electronegativity means between they

00:20:06

create a covalent polar bond, a

00:20:09

covalent non-polar bond

00:20:11

is realized between non-metal atoms with

00:20:15

the same electronegativity, we can

00:20:19

consider examples phosphorus chlorine hydrogen

00:20:22

sulfur oxygen these are either substances of atomic

00:20:26

structure or substances of molecular

00:20:27

structure, but the most important thing is that in the composition of

00:20:30

these substances there are

00:20:31

only one type of non-metal atoms and

00:20:35

how is it distributed here electron

00:20:39

pair electron density

00:20:41

we understand that both atoms in a molecule of,

00:20:44

for example, hydrogen or chlorine are absolutely the

00:20:46

same, which means that their

00:20:49

electronegativity is absolutely the

00:20:51

same, which means that none of the

00:20:54

atoms can pull over this

00:20:56

common electron pair

00:20:57

and it seems to remain in the middle between

00:21:00

two atoms, and if the pair does not shift,

00:21:03

then no

00:21:06

partial charges arise on the atoms, and

00:21:09

if no charges arise, then a

00:21:11

dipole is not formed, that is, there is no polarity,

00:21:15

and if there is no polarity, then the bond is

00:21:17

covalent, nonpolar, I think everything here is

00:21:19

very logical and simple, well Using a

00:21:24

graphic example, we can consider that the

00:21:26

electron densities

00:21:28

in the case of the formation of a covalent

00:21:31

nonpolar bond are distributed

00:21:34

very evenly and there is no

00:21:37

obvious shift to one side

00:21:40

because the atoms are the same and none of them

00:21:42

can pull this electron pair over themselves.

00:21:45

In which compounds is a

00:21:48

covalent bond realized? non-polar bond in all

00:21:51

simple substances of non-metals, it doesn’t matter if it’s not a

00:21:54

metal of atomic structure or not a metal of

00:21:56

molecular structure,

00:21:58

if this simple substance is not a metal,

00:22:01

it means it consists of atoms of only

00:22:04

one type and

00:22:06

of atoms of non-metals, and this is exactly the

00:22:09

option when a covalent

00:22:12

non-polar bond is realized,

00:22:13

that is, if this is a bond between non-metals,

00:22:16

this bond is covalent, if between

00:22:18

identical non-metals and in simple

00:22:20

substances they can only be the

00:22:21

same, then this is a covalent

00:22:24

non-polar bond,

00:22:26

I really hope that everything is clear here,

00:22:28

if it is not clear, you can ask

00:22:30

additional questions in the comments,

00:22:31

we will analyze it further, but you just need to

00:22:34

listen carefully, concentrate and

00:22:36

find out what a covalent bond is,

00:22:39

and the last thing we will talk about is what

00:22:43

crystal lattices are realized in

00:22:45

substances with a covalent bond; substances

00:22:48

with a covalent bond, we remember, there are both

00:22:52

atomic structure and molecular

00:22:55

structure; examples of substances of atomic

00:22:58

structure are simple substances non-metals

00:23:00

phosphorus sulfur silicon carbon and so in

00:23:04

crystalline in a lattice of substances with a

00:23:08

covalent bond of

00:23:09

atomic structure, substances of atomic

00:23:12

structure, at the lattice nodes there will be

00:23:15

individual neutral atoms,

00:23:18

this is, for example,

00:23:20

the crystal lattice of diamond, and this is the

00:23:24

crystal lattice of graphite, and here and

00:23:27

there at the lattice nodes there are only

00:23:30

carbon atoms, just a different

00:23:33

geometric arrangement of these atoms,

00:23:36

which is why diamond has and graphite have such

00:23:38

different physical and chemical properties,

00:23:40

but in general these are simple substances consisting

00:23:43

only of carbon atoms, naturally,

00:23:46

if a bond occurs between

00:23:48

non-metal atoms, carbon is not a metal, this

00:23:50

bond is covalent, well, taking into account the fact that

00:23:52

these atoms are absolutely identical in

00:23:55

electronegativity, this bond is

00:23:57

covalent, non-polar in substances

00:24:02

molecular structure, of course, at the

00:24:05

lattice sites there will be molecules,

00:24:08

for example, diatomic molecules chlorine 2 ooo

00:24:12

2

00:24:13

h2 n2 at the lattice sites these diatomic molecules are located,

00:24:18

here is another example, at the

00:24:21

lattice sites of water there will

00:24:23

be 3 atomic water molecules, that

00:24:26

is, we remember that there are three

00:24:29

types of bonds metallic covalent and

00:24:32

ionic which we will look at in the next

00:24:34

lesson and

00:24:36

there are 4 types of crystal lattices metallic

00:24:40

characteristic only for metals atomic

00:24:43

and molecular characteristic of substances with a

00:24:47

covalent bond and

00:24:49

ionic characteristic of course for

00:24:52

substances ionic bonds in more detail about the ionic

00:24:56

bond and the ionic crystal lattice

00:24:58

we We’ll talk in the next lesson,

00:25:00

but that’s all for today, if you still have

00:25:02

any questions, be sure to ask in

00:25:04

the comments, don’t forget to subscribe to the

00:25:06

channel and like

Description:

В этом уроке ты узнаешь, что такое химическая связь между атомами и почему она возникает. Существует три основных типа химической связи - металлическая, ковалентная, ионная. Ковалентная связь бывает полярной и неполярной.

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