Difference between Atoms and Ions (Explanation & Examples)

Summary

This video explains the key differences between atoms and ions, focusing on the role of electrons. Atoms are neutral, having equal protons and electrons, while ions have an imbalance due to gaining or losing electrons. The video uses examples like chlorine and nitrogen to show how atoms become negatively or positively charged ions through chemical bonding, particularly in ionic bonds. It also touches on periodic table trends, cations (positive ions), anions (negative ions), and polyatomic ions, making complex concepts simpler with clear visual examples.

Takeaways

• 🔬 Atoms and ions differ in the number of electrons, with ions having a charge due to an imbalance between protons and electrons.
• 🧪 Chlorine (Cl) is neutral in its atomic form, with equal numbers of protons and electrons.
• ⚛️ When chlorine gains an electron during chemical bonding, it becomes a negatively charged ion (Cl⁻).
• 🔋 Nitrogen, with an atomic number of 7, has 7 protons and 7 electrons in its neutral state.
• 💡 Ions are charged particles because the number of electrons does not equal the number of protons.
• ⚠️ Adding neutrons to the nucleus changes the atomic mass but not the charge of the atom or ion.
• ⚖️ Neutral atoms have equal numbers of protons and electrons, while ions do not.
• 📉 Nitrogen typically forms a 3⁻ ion because it gains 3 electrons to fill its outer shell.
• 🧲 Atoms that lose or gain electrons become ions and can form ionic bonds due to opposite charges (e.g., Na⁺ and Cl⁻).
• 📛 Cations are positively charged ions (e.g., Na⁺), while anions are negatively charged ions (e.g., Cl⁻).

Q & A

What is the main difference between an atom and an ion?

The main difference between an atom and an ion is the number of electrons. An atom is neutral, with an equal number of protons and electrons, while an ion has either gained or lost electrons, resulting in a charge.

Why is chlorine (Cl) considered a neutral atom?

Chlorine (Cl) is considered a neutral atom because the number of protons equals the number of electrons, which balances the positive and negative charges.

What happens when chlorine forms an ionic bond?

When chlorine forms an ionic bond, it gains an extra electron, resulting in a negative charge, making it a negatively charged ion (Cl⁻).

How do protons and electrons affect the charge of an atom or ion?

Protons are positively charged, and electrons are negatively charged. If an atom has an equal number of protons and electrons, it is neutral. If an atom has more electrons than protons, it becomes a negatively charged ion, and if it has fewer electrons, it becomes a positively charged ion.

What is the charge of a nitrogen ion, and why?

A nitrogen ion typically has a charge of 3⁻ because it gains three extra electrons to fill its outer shell, resulting in three more negative charges than positive protons.

How does the addition of neutrons affect the charge of an atom?

The addition of neutrons does not affect the charge of an atom. Neutrons are neutral particles, so they only change the atomic mass, not the charge.

What is the general trend for ions in Group 1 and Group 2 elements of the periodic table?

Group 1 elements, like sodium (Na), tend to lose one electron to form 1⁺ ions. Group 2 elements lose two electrons to form 2⁺ ions.

How are positive and negative ions (cations and anions) formed?

Positive ions (cations) are formed when an atom loses electrons, making it positively charged. Negative ions (anions) form when an atom gains electrons, giving it a negative charge.

What is an ionic bond, and how does it form between sodium and chlorine?

An ionic bond is the attraction between oppositely charged ions. It forms when sodium (Na) loses an electron to become Na⁺, and chlorine (Cl) gains that electron to become Cl⁻, resulting in the attraction between Na⁺ and Cl⁻ to form sodium chloride (NaCl).

What are polyatomic ions, and how do they get their charge?

Polyatomic ions are groups of atoms bonded together that have an overall positive or negative charge. They gain or lose electrons from other atoms, resulting in their charge.

Outlines

00:00

🔬 Understanding Atoms and Ions: The Role of Electrons

This paragraph introduces the concept of atoms and ions, emphasizing the role of electrons in differentiating between the two. Chlorine (Cl) is used as an example, where the neutral atom has equal numbers of protons and electrons. When chlorine gains an electron during bond formation, it becomes negatively charged and forms an ion. The key takeaway is that the imbalance between protons and electrons defines whether the particle is an atom (neutral) or an ion (charged).

05:02

🧪 Building a Nitrogen Atom and Ion

Here, nitrogen is used to demonstrate how atoms and ions are structured. With an atomic number of seven, nitrogen has seven protons and seven electrons in its neutral state, canceling out the charge. However, when nitrogen gains three electrons, it becomes an ion with a 3- charge. The explanation also covers how protons, neutrons, and electrons are arranged in energy levels and how adding neutrons affects the mass but not the charge. The key concept is the distinction between neutral atoms and ions, with a focus on electron gain or loss.

🧲 Determining Ions and Neutral Atoms from Periodic Table Trends

This section highlights how to distinguish between ions and neutral atoms, primarily using periodic table trends. If an atom has a charge (indicated by a plus or minus sign), it is an ion; otherwise, it's neutral. The periodic table provides clues to predict an atom's charge when it forms an ion. For example, nitrogen tends to form a 3- ion, while oxygen and sulfur form 2- ions. Elements like lithium and sodium lose electrons to become positive ions. These trends help simplify the prediction of ionic charges for various elements.

⚛️ Formation of Ionic Bonds: Sodium and Chlorine Example

This paragraph explains how ionic bonds form through electron transfer, using sodium (Na) and chlorine (Cl) as examples. Sodium loses an electron to become Na+, and chlorine gains an electron to become Cl-. The attraction between these opposite charges results in the formation of sodium chloride (NaCl). The section also briefly touches on ionization, where enough energy can remove electrons to form ions, although chemical bonding is more common in forming ions.

🔋 Cations, Anions, and Polyatomic Ions

The difference between cations (positive ions) and anions (negative ions) is introduced here. Cations form when atoms lose electrons, while anions form when atoms gain electrons. The paragraph offers mnemonic devices to remember these concepts, such as the 't' in cation resembling a plus sign. Additionally, the concept of polyatomic ions, groups of atoms with an overall charge, is briefly introduced. These polyatomic ions often bond with other elements and gain or lose electrons, resulting in a charge.

Keywords

💡Atom

An atom is the basic unit of matter, composed of protons, neutrons, and electrons. In the video, atoms are described as neutral entities where the number of protons (positively charged) equals the number of electrons (negatively charged), resulting in no overall charge. An example from the script is the chlorine atom (Cl), which is neutral before it gains or loses electrons.

💡Ion

An ion is an atom or molecule that has gained or lost one or more electrons, resulting in a net electrical charge. The video explains that when atoms like chlorine gain an electron, they become negatively charged ions (anions). Conversely, atoms that lose electrons become positively charged ions (cations), like sodium (Na+).

💡Electron

Electrons are negatively charged subatomic particles found outside the nucleus of an atom. In the video, the addition or removal of electrons is what transforms an atom into an ion. For instance, when chlorine gains an electron, it becomes a Cl- ion, while sodium loses an electron to become Na+.

💡Proton

Protons are positively charged particles found in the nucleus of an atom. The video emphasizes that in a neutral atom, the number of protons equals the number of electrons. For example, nitrogen has 7 protons, and in its neutral state, it also has 7 electrons.

💡Neutron

Neutrons are neutral (uncharged) subatomic particles found in the nucleus of an atom. In the video, neutrons are mentioned as contributing to the atomic mass but not affecting the charge of the atom. For example, nitrogen has 7 neutrons, and this contributes to its mass but not its charge.

💡Cation

A cation is a positively charged ion, formed when an atom loses one or more electrons. The video explains that sodium (Na) loses an electron to become Na+, a cation. The term 'cation' is emphasized by the visual cue that the 't' in cation looks like a plus sign, helping viewers remember the positive charge.

💡Anion

An anion is a negatively charged ion, formed when an atom gains one or more electrons. In the video, chlorine (Cl) gains an electron to become Cl-, an anion. The term 'anion' is connected with the word 'negative,' as anions carry a negative charge.

💡Ionic bond

An ionic bond is a type of chemical bond formed between two atoms with opposite charges. The video illustrates the formation of ionic bonds between sodium (Na+) and chlorine (Cl-), where sodium loses an electron and chlorine gains it, resulting in their attraction due to opposite charges, forming NaCl (sodium chloride).

💡Periodic table

The periodic table organizes elements by increasing atomic number and highlights patterns in their properties. The video references the periodic table to explain how elements like nitrogen, oxygen, and chlorine tend to form specific ions (e.g., nitrogen forms a 3- ion), and it also shows trends in ion formation based on an element's position.

💡Polyatomic ion

A polyatomic ion is a charged particle composed of two or more atoms covalently bonded, with an overall charge. The video briefly mentions polyatomic ions as groups of atoms that carry a charge, either positive or negative, and these ions frequently appear in chemical reactions, behaving as single charged entities.

Highlights

The key difference between atoms and ions revolves around electrons.

A neutral atom has an equal number of protons and electrons.

Chlorine (Cl) on the periodic table is neutral when the number of protons equals the number of electrons.

When chlorine gains an electron, it becomes an ion with a negative charge due to the excess electron.

Ions are charged particles, unlike neutral atoms, due to an imbalance in the number of protons and electrons.

Nitrogen has an atomic number of 7, meaning it has 7 protons, making it neutral when there are 7 electrons as well.

When nitrogen gains 3 electrons, it forms a 3- ion with a full outer shell, which is more stable.

Protons in the nucleus are positive, and neutrons stabilize the atom without affecting its charge.

A neutral nitrogen atom has a mass number of 14 due to its 7 protons and 7 neutrons.

Atoms become ions when the number of electrons and protons are unequal.

Elements in certain periodic table groups tend to form ions with predictable charges (e.g., nitrogen forms a 3- ion).

Metals like sodium (Na) lose electrons to form positive ions (cations), while nonmetals like chlorine gain electrons to form negative ions (anions).

Ions with opposite charges (e.g., Na+ and Cl-) attract each other to form ionic bonds, like in sodium chloride (NaCl).

Ionization can occur by removing electrons through chemical bonding or by adding energy to atoms.

Cations are positive ions (e.g., Na+), and anions are negative ions (e.g., Cl-), with a simple way to remember: 'a negative ion' for anions.

Polyatomic ions are groups of atoms with an overall charge, often found in chemical compounds.

Transcripts

in this video we'll talk about the

difference between atoms and ions and

when we're talking about the difference

between atoms and ions it's all about

the electrons

let's take a look at an example of this

so if we have an atom like chlorine on

the periodic table cl

that's considered to be neutral that's

because the number of protons and the

number of electrons in the atom they're

equal so this is an atom and because

there's no plus or minus after it it's

considered to be neutral and the number

of protons will equal the number of

electrons

but chlorine forms chemical bonds and

when it forms chemical bonds ionic bonds

it tends to gain an electron electrons

are negative so then we have this

negative sign here so now we consider

this to be

an ion

and with an ion it's charged it's not a

neutral particle it has a charge it has

a negative charge here because it has an

extra electron and in this case we say

that the protons they don't equal the

number of electrons we have one more

electron than we have protons so this

charge the difference in electrons that

makes this an ion so let's see what that

really looks like

so let's build an atom and an ion so

let's work with nitrogen nitrogen on the

periodic table that has an atomic number

of seven so it has seven protons let's

add seven protons

protons they're found in the nucleus

here

they are positive

so we have 7 protons seven positive

charges so this is an ion because it has

a positive charge in fact it has a seven

plus charge because we have seven

protons and they're positive

we said that a neutral atom like those

found on the periodic table doesn't have

a plus or minus after it the electrons

will equal the protons so the electrons

which are negative

if we have seven of those that would

cancel out the positive that would give

us a net charge of zero it would be

neutral we put 2 in the first energy

level and then 5 more in the second

energy level

so we have 7

electrons and 7 protons

the net charge is zero this is a neutral

atom

but you'll notice something interesting

there's space for more electrons here in

this outer shell so we could add three

more here

to fill this shell

so now we have a full outer shell which

is really stable and our nitrogen ion

would have a charge of 3 minus and

that's the charge we get when nitrogen

forms ionic bonds

we should probably put some neutrons in

here too these protons are positive

they're going to push away from each

other so let's put seven neutrons in

and you'll notice nothing happens when

we put neutrons in to the charge

the only thing that's changing here is

the atomic mass so this would be the

most common isotope of nitrogen here

you'd have a mass number of 14 because

we have seven neutrons and protons but

when we talk about atoms and ions

we have three extra electrons we have a

three minus charge this is an ion

but if the number of electrons and

protons are equal we call it a neutral

atom

so pause and determine which of the

following are ions and which are neutral

atoms

so if you have a plus or minus after

them they're going to be ions if there's

nothing written that's a neutral atom

and the number of protons will equal the

number of electrons and if you have just

a minus that means it's one minus

there's a general trend on the periodic

table we can follow to tell what the

charge will be on atoms when they become

ions so nitrogen that's right here on

the periodic table so nitrogen will have

a three minus in fact the elements here

in general will form ions that are three

minus and note we write the plus or the

minus after the number when we're

dealing with ions just the way we do it

if we have something here like oxygen or

sulfur

form two minus ions things like fluorine

chlorine

those will form one minus ions if you

came over here and you looked at lithium

or sodium they would tend to lose an

electron to form ions

elements in group two they lose two

electrons we don't include the

transition metals they can have

different charges depending what they

bond to

this is a general way we can look at how

atoms when they form ions what their

charge will be

we can be a little more specific if we

look at this periodic table here you can

see that some of these really we can't

look at ionic charges for but these are

the general trends and if you know these

chemistry gets a lot easier

so you might ask how does an atom become

an ion well sodium has one electron in

its outer shell it'll lose that electron

when it forms a chemical bond with

chlorine so sodium ends up having a one

plus ionic charge

the chlorine which gained that electron

it now has an extra electron right here

so now it has a negative charge and you

have this plus and minus these two atoms

with opposite charges they're going to

be attracted and they're going to form

an ionic bond they're going to come

together and be attracted to form this

nacl sodium chloride so the plus

and the minus

comes when they form bonds

there is one other way you can do this

if you have just solid sodium or another

atom and you hit it with enough energy

you can remove electrons to form ions

this is called ionization

but most of the time in chemistry we're

dealing with chemical bonds and with

ions they'll form when we have a metal

coming together with a non-metal forming

that ionic

bond so we've talked about positive ions

like na plus or ca2 plus these are

called cations and the way you can

remember is the t here looks like a plus

sign

we also had negative ions they're called

anions like cl minus or n3 minus the way

i like to remember those is a

negative

ion so anions a negative ion that'll

help you remember that they're negative

the cations they lost an electron that

made them positive the anions they've

gained electrons so they become negative

neutral elements like we find on the

periodic table they have the same number

of protons and electrons

one last thing sometimes you'll see

groups of atoms together with a charge

negative or a positive charge after them

these are considered polyatomic ions

they're made up of groups of atoms

together and they have an overall charge

we see these quite often in chemistry

bonded to other elements in fact they

get their charge because they're bonded

to an element that loses electrons they

gain them they have the negative charge

this is dr b with the difference between

atoms and ions thanks for watching