Introduction to Atoms Flashcards

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1
Q

What is an Atom?

A

The basic building blocks of matter
The smallest particles of an element that retain the chemical properties of that element
Combine to form molecules which make up al substances

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2
Q

What is the structure of an atom?

A

Three main subatomic particles
Proton, Neutrons, Electrons
Protons + Neutrons are found in the center = Nucleus
Electrons orbit the nucleus in energy levels/shells

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3
Q

Protons

A

Have a + charge and contribute to the mass of the atom

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4
Q

Neutrons

A

Have no charge and contribute to the mass of the atom

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5
Q

Electrons

A

Have a - charge and are much smaller in mass

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6
Q

What is the Atomic number?

A

The number of protons in an atom

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7
Q

What is the Atomic mass?

A

The sum of the protons and neutrons in the nucleus

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8
Q

What is an Isotope?

A

Atoms of the same element with different numbers of neutrons

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9
Q

What are Electron Shells?

A

Electrons occupy specific energy levels or shells around the nucleus
Inner most shell hold up to 2 electrons, second holds up to 8
Outermost shell is know as valence shell - determine the chemical behaviour of an atom

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10
Q

Valence electrons

A

Electrons in the outermost shell
The number influences how atoms interact with each other in chemical reactions
Elements in the same group of the periodic table have similar valence electron configurations

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11
Q

Definition of Elements

A

Substances made up of only one type of atom
Cannot be broken down into simpler substances by chemical means

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12
Q

Examples of Elements

A

Oxygen (O)
Hydrogen (H)
Carbon (C)

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13
Q

Properties of Elements

A

Each element has its own unique set of physical & chemical properties
Elements are organized in the periodic table based on their properties

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14
Q

Definition of compounds

A

Substance made up of two or more different types of atoms chemically bound together
Can be broke down into simpler substances by chemical means

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15
Q

Examples of Compounds

A

Water (H2O)
Carbon dioxide (CO2)
Sodium Chloride (NaCl)

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16
Q

Properties of Compounds

A

Compound often have properties different from elements that make them up
The ratio of atoms is fixed
Attraction between particles is called intermolecular force of attraction
This force keeps the particles of matter held together

17
Q

Definition of Covalent Bonds

A

When atoms share electrons to achieve a stable electron configuration
Typically occurs between non-metal atoms

18
Q

Examples of Covalent Bonds

A

Formation of water molecule (H2O) where each hydrogen atom share its electron with the oxygen atom

19
Q

Properties of Covalent Bonds

A

Strong within molecules but weak between molecules
They have lower melting & boiling point than ionic bonds

20
Q

Name 3 types of Covalent Bonds

A

Single
Double
Triple

21
Q

Definition of Ionic Bond

A

Form when one atom transfers electrons to another to achieve a stable electron configuration
Typically occur between metal & non-metal atoms

22
Q

Examples of Ionic Bonds

A

Formulation of sodium chloride (NaCl) where sodium loses an electron to chlorine, resulting in opposite charged ions (Na+, Cl-) that attract eachother

23
Q

Properties of Ionic Bonds

A

Strong electrostatic force of attraction between ions
Often from crystalline structures with high melting and boiling points

24
Q

Formation of Ionic Bonds

A

Metal tend to lose electrons to form + charged ions (Cations)
Non-metal tend to gain electrons to form - charged ions (Anions)

25
Q

Compound formed by ions bonds are called what?

A

Salts