Name: atomic elements, molecules, and bonds
Uploaded: 2020-09-03T13:38:25.000Z
Duration: 2 min 38 s
Channel: JoVE

K12 Standards

north-carolina-k-12-science-standard-course-of-study

North Carolina K-12 Science Standard Course of Study

9-12

Chemistry

Matter and its Interactions

PS.Chm.3.3

Molecules and Compounds

W przyrodzie cała materia składa się z podstawowych jednostek chemicznych zwanych pierwiastkami o określonych właściwościach fizycznych i chemicznych.

Układ okresowy pierwiastków zawiera w sumie 118 zidentyfikowanych do tej pory pierwiastków. Jednostką składową każdego pierwiastka jest atom. Niektóre pierwiastki, takie jak hel, neon, srebro lub platyna, istnieją jako jednostki niezależnych pojedynczych atomów.

Inne pierwiastki, takie jak wodór, tlen lub siarka, istnieją jako jednostki dwóch lub więcej identycznych atomów. Te wielokrotne atomy są utrzymywane razem przez silne siły elektrostatyczne zwane wiązaniami chemicznymi, tworząc stabilne jednostki zwane cząsteczkami.

Ponadto dwa lub więcej różnych pierwiastków może również łączyć się, tworząc cząsteczki, takie jak woda lub fruktoza. Takie cząsteczki, które powstają w wyniku połączenia atomów dwóch lub więcej pierwiastków, połączonych chemicznie w ustalonej proporcji, nazywane są również związkami. W związku z tym cząsteczki wody i fruktozy są również związkami.

Woda to cząsteczka zbudowana z dwóch atomów wodoru i jednego atomu tlenu. Natomiast fruktoza to cząsteczka zawierająca sześć atomów węgla, dwanaście atomów wodoru i sześć atomów tlenu.

Poszczególne atomy w związku są utrzymywane razem przez wiązania chemiczne, co dyktuje rodzaj powstającego związku, takiego jak związek molekularny lub jonowy.

Związki kowalencyjne lub molekularne, takie jak woda, powstają, gdy atomy niemetalu łączą się i dzielą swoje elektrony walencyjne za pośrednictwem wiązania kowalencyjnego. Wspólne elektrony między dwoma atomami obniżają energię potencjalną i tworzą bardziej stabilne cząsteczki w porównaniu z pojedynczymi atomami.

Związki jonowe, takie jak chlorek sodu, powstają, gdy atomy metalu i niemetalu spotykają się ze sobą. Metale łatwo tracą elektrony, stając się kationami, podczas gdy niemetale łatwo zyskują elektrony, stając się anionami. W ten sposób atomy metalu przenoszą elektrony na atomy niemetali, a oddziaływania elektrostatyczne między przeciwnie naładowanymi jonami tworzą wiązania jonowe.

Zdolność pierwiastków do tworzenia związków przyczynia się do wielkiej różnorodności materii występującej w przyrodzie.

cząsteczki i związki

<h4>Atomy i cząsteczki</h4>

Wszystko we wszechświecie składa się z materii, a materia składa się z połączeń pierwiastków. Atom to najmniejsza jednostka pierwiastka, która zachowuje wszystkie jego właściwości. Na przykład srebrna moneta składa się z atomów srebra, a każdy atom srebra zachowuje unikalne właściwości pierwiastka – srebra.

Pierwiastki to czyste substancje składające się z identycznych atomów, których nie można rozłożyć na prostsze substancje w wyniku przemian chemicznych. Pierwiastki atomowe zawierają pojedyncze atomy jako podstawową jednostkę. Węgiel składa się z atomów węgla, a sód z atomów sodu. Większość pierwiastków to pierwiastki atomowe. Istnieje jednak kilka pierwiastków, które stanowią kombinację atomów i nigdy nie występują w przyrodzie jako pojedyncze atomy. Nazywa się je pierwiastkami cząsteczkowymi. Pierwiastki takie występują jako cząsteczki z dwoma lub większą liczbą połączonych ze sobą atomów. Mogą być dwuatomowe, jak wodór (H2), tlen (O2) lub gazowy chlor (Cl2), lub wieloatomowe, jak siarka (S8) i fosfor (P4).

Cząsteczka składa się z dwóch lub więcej atomów połączonych znacznymi siłami zwanymi wiązaniami chemicznymi. Cząsteczka może składać się z dwóch lub więcej identycznych atomów lub może składać się z dwóch lub więcej różnych atomów. Kiedy cząsteczka składa się z atomów dwóch lub więcej różnych pierwiastków, połączonych w ustalonych proporcjach liczb całkowitych, jest również związkiem. Na przykład woda jest związkiem, a każda cząsteczka wody (H2O) jest jednostką zawierającą dwa atomy wodoru i jeden atom tlenu. Cząsteczka glukozy (C6H12O6) jest również związkiem zawierającym sześć atomów węgla, dwanaście atomów wodoru i sześć atomów tlenu.

Związki to czyste substancje składające się z dwóch lub większej liczby pierwiastków w ustalonych, określonych proporcjach. Związki klasyfikuje się jako molekularne lub jonowe na podstawie występujących wiązań.

<h4>Związki</h4>

Charakter sił przyciągających utrzymujących razem atomy w związku, decyduje o rodzaju utworzonego wiązania chemicznego. Całkowite przeniesienie elektronów pomiędzy atomem metalu i atomem niemetalu powoduje powstanie przeciwnie naładowanych jonów. Przyciąganie elektrostatyczne między jonami nazywa się wiązaniem jonowym, a związki utworzone przez wiązania jonowe są związkami jonowymi. Na przykład chlorek sodu NaCl jest związkiem jonowym.

Współdzielenie elektronów przez dwa lub większą liczbę atomów niemetalu skutkuje powstaniem wiązań kowalencyjnych, a związki utworzone przez wiązania kowalencyjne nazywane są związkami kowalencyjnymi lub molekularnymi. Wiązania kowalencyjne to siły przyciągania pomiędzy dodatnio naładowanymi jądrami związanych atomów i ujemnie naładowanymi elektronami współdzielonymi pomiędzy atomami.

Cząsteczki i związki

Atomy i cząsteczki

Wszystko we wszechświecie składa się z materii, a materia składa się z kombinacji pierwiastków. Atom to najmniejsza jednostka ...

Education

JoVE Core

Chemia

Jeden

Molecules, Compounds, and Chemical Equations

Cząsteczki, związki chemiczne i równania chemiczne

molecules-compounds-and-chemical-equations

KEY TERMS AND CONCEPTS

Kluczowe terminy i pojęcia

atomic elements, molecules, and bonds

Matter is made of elements, and elements are built from atoms. An atom is the smallest unit of an element that still keeps that element’s properties. A silver coin, for example, is made of silver atoms. Each atom keeps the unique properties of silver.

Elements are pure substances made of identical atoms. They cannot be broken down into simpler substances by chemical changes. Most elements are atomic elements, which use single atoms as their basic unit. Carbon and sodium are examples of atomic elements.

Some elements do not occur as single atoms in nature. These are called molecular elements. They exist as molecules made of two or more bonded atoms. Some are diatomic, such as hydrogen (H2), oxygen (O2), and chlorine (Cl2). Others are polyatomic, such as sulfur (S8) and phosphorous (P4).

A molecule is a group of two or more atoms joined by strong chemical bonds. The atoms in a molecule may be the same, or they may be different. When a molecule contains atoms from two or more different elements in fixed whole number ratios, it is also a compound. Water is a compound, and each H2O molecule has two hydrogen atoms and one oxygen atom. Glucose (C6H12O6) is another compound, with six carbon atoms, twelve hydrogen atoms, and six oxygen atoms.

Compounds are pure substances made of two or more elements in fixed, definite proportions. They are classified as molecular or ionic based on the bonds they contain. The kind of attraction between atoms determines the bond type. When electrons transfer completely from a metal atom to a nonmetal atom, oppositely charged ions form. The electrostatic attraction between those ions is an ionic bond, and the result is an ionic compound such as sodium chloride (NaCl). When two or more nonmetal atoms share electrons, they form covalent bonds. Compounds formed this way are covalent, or molecular, compounds.

Atomic Elements, Molecules, and Bonds

molecules and compounds

Matter is made of elements, and elements are built from atoms. An atom is the smallest unit of an element that still keeps that element’s properties. A silver coin, for example, is made of silver atoms. Each atom keeps the unique properties of silver. Elements are pure substances made of identical atoms. They cannot be broken down into simpler substances by chemical changes. Most elements are atomic elements, which use single atoms as their basic unit. Carbon and sodium are examples of atomic...

molecular models

Molecular Model Types in Chemistry

Molecular models help chemists and students visualize the structures and shapes of atoms and molecules. They represent the molecular architecture of chemical compounds in a way that is easier to study than formulas alone. Skeletal models are simple two-dimensional drawings of compounds. They show the molecular framework, or the bonds, without drawing every atom. In this model, many carbon and hydrogen atoms are not shown directly. Their positions are implied by the ends and junctions of the...

organic compounds

Organic Molecules in Everyday Chemistry

Organic molecules are carbon-based compounds found in living things and in many everyday products. Most organic compounds have carbon as the main element, bonded to hydrogen and other carbon atoms. Some carbon-containing substances, such as carbonates, cyanides, and simple oxides like CO and CO2, are not classified as organic. Carbon can form up to four strong bonds, which helps explain why organic compounds can make chains and rings of many sizes and shapes. These molecules appear in...

formula mass and mole concepts of compounds

formula-mass-and-mole-concepts-of-compounds

Chemical Formula Mass and Percent Composition

Chemical formula mass and percent composition help describe the makeup of compounds. A chemical formula shows which atoms are present and how many of each atom appear in a substance. For covalent compounds, the formula shows the atoms in one molecule. That is why formula mass can also be called molecular mass. Chloroform, CHCl3, is one example. Its formula shows one carbon atom, one hydrogen atom, and three chlorine atoms. The molecular mass is the sum of their average atomic masses. Ionic...

experimental determination of chemical formula

experimental-determination-of-chemical-formula

Finding Empirical and Molecular Formulas

Chemical formulas show the elemental makeup of a compound. When a formula is unknown, scientists often start by measuring the masses of the elements in the sample. Those mass data are then used to find the simplest whole-number ratio of atoms, which gives the empirical formula. To get from mass to atom ratio, the masses of the elements are first converted to moles using molar masses. Chemical formulas describe numbers of atoms, not masses, so this step is necessary. In one example, 1.71 grams...

chemical equations

Reading Chemical Equations and Balancing Them

Chemical equations show the identities and relative amounts of substances in a chemical reaction. The substances that react are called reactants, and their formulas are written on the left side of the equation. The substances formed are called products, and their formulas are written on the right side. A plus sign (+) separates formulas on the same side, and an arrow (→) shows the change from reactants to products. The numbers in a chemical equation are shown with coefficients. A coefficient...

key terms and concepts

Learn how atoms form elements, molecules, and compounds, and compare ionic and covalent bonds using examples like water, glucose, and sodium chloride.

Atomic Elements, Molecules, and Bonds | JoVE K12

chemistry

JoVE Core Chemistry brings general chemistry concepts to life using concise and easy-to-understand animated video lessons. Plus, in the scientist-in-action videos, we demonstrate classical and original research experiments performed in today's laboratories worldwide.

PS.Chm.4.3

Physical Science

PS.PSc.1.1

ohios-learning-standards-and-model-curriculum

Ohio’s Learning Standards and Model Curriculum

Study Of Matter

Classification of matter

Virginia  Standards of Learning

HIgh School

CH.3

CH.3.a

Alabama Course of Study Science

Matter and Its Interactions

9-12.PS.3.4.c

south-carolina-college-and-career-ready-science-standards

South Carolina College and Career Ready Science Standards

High School

C-PS1-3.

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Motion and Stability: Forces and Interactions

C-PS2-6.

Scientific Laws and Theories

Scientific Laws

In science, a law is defined as a concise, verbal or mathematical, statement that summarizes a vast number of experimental observations. ...

The Scientific Method

Chemistry is an empirical science. Scientists often pose questions to understand the chemistry in everyday life and seek answers to these questions. To ...

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Chemistry is the study of matter and the changes it undergoes. Matter is anything that has mass and occupies space. Matter is all around us; the air, ...

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Matter: Pure Substances and Mixtures
According to its composition, the matter can be classified into two broad categories &mdash; pure substances and ...

The Atomic Theory of Matter

The earliest recorded discussion of the basic structure of matter comes from ancient Greek philosophers. Leucippus and Democritus argued that all matter ...

Subatomic Particles

Dalton was only partially correct about the particles that make up matter. All matter is composed of atoms, and atoms are composed of three smaller ...

Elements: Chemical Symbols and Isotopes

A chemical symbol is an abbreviation used to indicate an element or an atom of an element. For example, the symbol for mercury is Hg. The same symbol is ...

Use models to explain how the scientific understanding of atomic structure has evolved.

PS.Chm.1.1

Radioactivity and Nuclear Equations

Nuclear chemistry is the study of reactions that involve changes in nuclear structure. The nucleus of an atom is composed of protons and, except for ...

Types of Radioactivity

The most common types of radioactivity are &#945; decay, &#946; decay, &#947; decay, neutron emission, and electron capture.
Alpha (&#945;) decay is the ...

Nuclear Stability

Protons and neutrons, collectively called nucleons, are packed together tightly in a nucleus. With a radius of about 10&#8722;15 meters, a nucleus is ...

Nuclear Binding Energy

The difference between the calculated and experimentally measured masses is known as the mass defect of the atom. In the case of helium-4, the mass defect ...

Radioactive Decay and Radiometric Dating

Radioactivity is a spontaneous disintegration of an unstable nuclide and is a random process, as all the nuclei in the sample do not decay simultaneously. ...

Nuclear Fission

Many heavier elements with smaller binding energies per nucleon can decompose into more stable elements that have intermediate mass numbers and larger ...

Nuclear Power

Controlled nuclear fission reactions are used to generate electricity. Any nuclear reactor that produces power via the fission of uranium or plutonium by ...

Nuclear Fusion

The process of converting very light nuclei into heavier nuclei is also accompanied by the conversion of mass into large amounts of energy, a process ...

Nuclear Transmutation

Nuclear transmutation is the conversion of one nuclide into another. It can occur by the radioactive decay of a nucleus, or the reaction of a nucleus with ...

Use models to compare nuclear reactions including alpha decay, beta decay and gamma decay; nuclear fusion and nuclear fission.

PS.Chm.1.2

Atomic Orbitals

An atomic orbital represents the three-dimensional regions in an atom where an electron has the highest probability to reside. The radial distribution ...

The Pauli Exclusion Principle

The arrangement of electrons in the orbitals of an atom is called its electron configuration. We describe an electron configuration with a symbol that ...

The Energies of Atomic Orbitals

In an atom, the negatively charged electrons are attracted to the positively charged nucleus. In a multielectron atom, electron-electron repulsions are ...

The Aufbau Principle and Hund's Rule

To determine the electron configuration for any particular atom, we can build the structures in the order of atomic numbers. Beginning with hydrogen, and ...

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Electron Configuration of Multielectron Atoms

The alkali metal sodium (atomic number 11) has one more electron than the neon atom. This electron must go into the lowest-energy subshell available, the ...

Use models to explain how electrons are distributed in atoms.

PS.Chm.1.3

Periodic Classification of the Elements

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The Periodic Table

As early chemists discovered more elements, they realized that various elements could be grouped by their similar chemical behaviors. One such grouping ...

Atomic Mass

Atoms &mdash; and the protons, neutrons, and electrons that compose them &mdash; are extremely small. For example, a carbon atom weighs less than 2 ...

Molar Mass

The identity of a substance is defined not only by the types of atoms or ions it contains but by the quantity of each type of atom or ion. For example, ...

Use the Periodic Table as a model to predict the relative properties of elements based on the pattern of valence electrons in the outermost energy levels of atoms.

PS.Chm.2.1

atomic-radii-and-effective-nuclear-charge

Atomic Radii and Effective Nuclear Charge

The elements in groups of the periodic table exhibit similar chemical behavior. This similarity occurs because the members of a group have the same number ...

Ionic Radii

Ionic radius is the measure used to describe the size of an ion. A cation always has fewer electrons and the same number of protons as the parent atom; it ...

Ionization Energy

The amount of energy required to remove the most loosely bound electron from a gaseous atom in its ground state is called its first ionization energy ...

Electron Affinity

The electron affinity (EA) is the energy change for adding an electron to a gaseous atom to form an anion (negative ion).



This process can be either ...

Construct an explanation to infer the atomic size, reactivity, electronegativity, and ionization energy of an element based on its position in the Periodic Table.

PS.Chm.2.2

Types of Chemical Bonds

Chemical bonding theories were pioneered by American chemist Gilbert&#xA0;N. Lewis. He developed a model called the Lewis model to explain the type and ...

Lewis Symbols and the Octet Rule

Chemical bonds are complex interactions between two or more atoms or ions, which reduce the potential energy of the molecule. Gilbert N. Lewis developed a ...

Ionic Bonding and Electron Transfer

Ions are atoms or molecules bearing an electrical charge. A cation (a positive ion) forms when a neutral atom loses one or more electrons from its valence ...

The Born-Haber Cycle

Lattice Energy&#xA0;

An ionic compound is stable because of the electrostatic attraction between its positive and negative ions. The lattice energy of a ...

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Trends in Lattice Energy: Ion Size and Charge

An ionic compound is stable because of the electrostatic attraction between its positive and negative ions. The lattice energy of a compound is a measure ...

Covalent Bonding and Lewis Structures

Compared to ionic bonds, which results from the transfer of electrons between metallic and nonmetallic atoms, covalent bonds result from the mutual ...

Electronegativity

Whether a bond is nonpolar or polar covalent is determined by a property of the bonding atoms called electronegativity.&#xA0;

Electronegativity values of ...

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Bond Polarity, Dipole Moment, and Percent Ionic Character

Bond Polarity

The absolute value of the difference in electronegativity (&Delta;EN) of two bonded atoms provides a rough measure of the polarity to be ...

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Lewis Structures of Molecular Compounds and Polyatomic Ions

To draw Lewis structures for complicated molecules and molecular ions, it is helpful to follow a step-by-step procedure as outlined:


	Determine the ...

Resonance

The Lewis structure of a nitrite anion (NO2&minus;) may actually be drawn in two different ways, distinguished by the locations of the N-O and N=O ...

Formal Charges

In some cases, there are seemingly more than one valid Lewis structures for molecules and polyatomic ions. The concept of formal charges can be used to ...

Exceptions to the Octet Rule

Many covalent molecules have central atoms that do not have eight electrons in their Lewis structures. These molecules fall into three categories:


	...

Bond Energies and Bond Lengths

Stable molecules exist because covalent bonds hold the atoms together. The strength of a covalent bond is measured by the energy required to break it, ...

Analyze and interpret data to explain the mechanisms and properties of the two main types of intramolecular (ionic and covalent) bonds.

PS.Chm.3.1

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Molecular Comparison of Gases, Liquids, and Solids

Particles in a solid are tightly packed together (fixed shape) and often arranged in a regular pattern; in a liquid, they are close together with no ...

Intermolecular vs Intramolecular Forces

Intermolecular forces (IMF) are electrostatic attractions arising from charge-charge interactions between molecules. The strength of the intermolecular ...

Intermolecular Forces

Atoms and molecules interact through bonds (or forces): intramolecular and intermolecular. The forces are electrostatic as they arise from interactions ...

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Comparing Intermolecular Forces: Melting Point, Boiling Point, and Miscibility

Intermolecular forces are attractive forces that exist between molecules. They dictate several bulk properties, such as melting points, boiling points, ...

surface-tension-capillary-action-and-viscosity

Surface Tension, Capillary Action, and Viscosity

Surface Tension
The various IMFs between identical molecules of a substance are examples of cohesive forces. The molecules within a liquid are surrounded ...

Hydrogen Bonds

Hydrogen BondsHydrogen bonds are weak attractions between atoms that have formed other chemical bonds. One of these atoms is electronegative, like oxygen, ...

Van der Waals Interactions

Atoms and molecules interact with each other through intermolecular forces. These electrostatic forces arise from attractive or repulsive interactions ...

Construct an explanation to summarize the influences intermolecular forces have on the properties of chemical compounds.

PS.Chm.3.2

Atoms and Molecules

Everything in the universe is made up of matter, and matter is composed of a combination of elements. An atom is the smallest unit of ...

Chemical Formulas

A chemical formula presents information about the proportions of atoms constituting a particular chemical compound or molecule, mainly using symbols of ...

Molecular Models

Physical models representing molecular architectures of chemical compounds play essential roles in understanding chemistry. The use of molecular models ...

Classification of Elements and Compounds

Pure substances consist of only one type of matter. A pure substance can be an element or a compound. An element consists of only one type of atom, while ...

ionic-compounds-formulas-and-nomenclature

Ionic Compounds: Formulas and Nomenclature

An element composed of atoms that readily lose electrons (a metal) can react with an element composed of atoms that readily gain electrons (a nonmetal) to ...

molecular-compounds-formulas-and-nomenclature

Molecular Compounds: Formulas and Nomenclature

Molecular compounds or covalent compounds result when atoms share electrons to form covalent bonds. Since there is no electron transfer, molecular ...

Use models to predict chemical names and formulas including ionic (binary & ternary), acidic, and binary covalent compounds.

Analyze the structure of atoms and isotopes.

Atomic Elements, Molecules, and Bonds

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