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Chemistry > 2.5 Simple molecules and covalent bonds > Flashcards

2.5 Simple molecules and covalent bonds Flashcards

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1
Q

molecule

A

a group of atoms bonded together representing the smallest fundamental unit of a chemical compound that can take part in a chemical reaction

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2
Q

covalent bonds are held together by

A

weak intermolecular forces

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3
Q

Properties of covalent bonds

A

low melting and boiling point
Poor conductivity
insoluble

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4
Q

Covalent bond

A

When two or more non-metal atoms bond together. The atoms need more electrons to fill their outer shell, so they share to complete

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5
Q

Covalent bonds have these properties because

A

They have low melting and boiling points because of the weak intermolecular forces holding them together

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6
Q

Compound

A

A substance is made of two or more elements chemically bonded.
It has a definite composition

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7
Q

Mixture

A

A substance made of two or more substances physically combined.
It has variable composition

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8
Q

Element

A

A substance made of only one type of atom

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9
Q

Proton number/atomic number

A

Is equal to the number of protons

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10
Q

Electron

A

A negatively charged subatomic particle that orbits the nucleus

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11
Q

Atom structure

A

An atom contains a central nucleus containing neutrons and protons surrounded by electrons in shells

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12
Q

Group number

A

Represents the number of electrons in the outer shell

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13
Q

Mass number/nucleon number

A

Is equal to the total number of protons and neutrons in the nucleus of the atom

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14
Q

Proton

A

a positively charged subatomic particle found in the nucleus

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15
Q

Periodic number

A

Represents the number of electron shells

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16
Q

How to determine the electron configuration

A

Proton number= Electron number
Electron configuration goes up first in 2 in the first shell then the rest 8 2.8.8.8.

17
Q

Neutron

A

A neutrally charged subatomic particle found in the nucleus

18
Q

Calculate the relative atomic mass

A

It is the sum of (atomic mass x relative abundance) for each Isotope dived by the sum of the relative abundance.(100)

19
Q

Isotope

A

Atoms of the same element so they have the same number of protons but with a different number of nuetrons

20
Q

Why do ionic bonds have these properties

A

They have high melting and boiling points because they are held together with strong electrostatic forces in lattice of positive and negative ions
They can conduct in liquid solutions because the ions become free to move

21
Q

Ion

A

An electrically charged particle formed when an atom either loses or gains electrons.

22
Q

Anion

A

Negatively charged ion

23
Q

Cation

A

positively charged ion

24
Q

Properties of ionic compounds

A

High boiling and melting points
Good electrical conductivity when aqueous or molten and poor when solid.

25
Q

Ionic bond

A

A force of attraction between a cation and an anion (between metals and nonmetals)

26
Q

What are the similarities between diamond, silicon and graphite

A

High melting point as a lot of energy is needed to break the strong covalent bonds

27
Q

Macromolecule

A

A giant molecule created by atoms covalently bonded to one another

28
Q

What are the properties and structure of diamond

A

Made of carbon with 4 covalent bonds
Is the hardest substance on earth because of it using all of its bonds

29
Q

The properties and structure of graphite

A

Is made of carbon and each atom makes 3 bonds
Used as a lubricant because the layers in the structure can slide over each other because they are only held together by weak intermolecular forces
Can conduct electricity because of one delocalised electron

30
Q

The three most know macromolecules

A

Diamond
Graphite
Silicon

31
Q

The properties and structures of silicon

A

Made of silicon and oxygen atoms in the ratio SiO2 in the same structure as diamond
High melting point

32
Q

Metallic bonding

A

There are strong electrostatic attractions
between the positive metal ions (cations) and
the negative delocalised electrons

33
Q

Melting and boiling points in metals

A

As the metallic lattice is held together by strong electrostatic forces of attraction, metals have high melting points and boiling points.

34
Q

Electrical conductivity in metals

A

The delocalised electrons in the metallic lattice are free to move throughout the structure and so metals are good at conducting electricity.

35
Q

Malleability and ductility of metals

A

Metals are malleable and ductile

Chemistry (12 decks)

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