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Chemistry ✏️ > 3. Atoms, Elements And Compounds > Flashcards

3. Atoms, Elements And Compounds Flashcards

0
Q

Define isotope

A

Atoms of the same element with different numbers of neutrons ( and nucleon numbers)

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1
Q

What is the relative mass of electron?

A

1/1804

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2
Q

One medical use of radioactive isotopes

A

Cancer treatment - radiation given out by the radioisotopes is used to kill cancer cells (cobalt-60)

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3
Q

One industrial use of isotopes

A

Check for leaks in oil and gas pipeline

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4
Q

Describe Noble Gas

A

They have full outer shell of electrons and so very stable
The atom cannot gain or lose electrons very easily
They are unreactive because their stability of a full outer shell
Colorless gas
Do not combine with other elements to form compound

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5
Q

Define element

A

A substance made of only one type of atom

They cannot broken down into anything simpler by chemical reacrion

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6
Q

What is chemical bond?

A

Link joining the atoms

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7
Q

Define compound

A

A substance made up of two or more different types of atoms joined together by chemical bonds
Cannot physically separate the elements in a compound

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8
Q

Define mixture

A

Contains two or more elements or compounds that are not chemically bonded together
The substances in a mixture can be separated physically

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9
Q

Properties of metals

A 
Conducts electricity and heat
Malleable
Ductile
Lustrous
Sonorous
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10
Q

Properties of non-metals

A 
Does not conduct heat or electricity
Not malleable or ductile - brittle
Dull surface
Not sonorous
Lower MP&BP than metal
Low density
Form negatively charged ions
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11
Q

Define alloy

A

Mixture of two or more elements where at least one element is a metal

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12
Q

Properties of alloys

A

Improve its properties
The other substance is often a metal
Alloys contain atoms of different size so it distorts the regular arrangement of atoms
This makes it more difficult for the layers to slide over each other => alloys are harder than the pure metal

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13
Q

Define ions

A

Charges atom

Number of protons are not equal to the number of electron

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14
Q

What is cations

A

Positively charged atom, usually metal

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15
Q

What is anion

A

Negatively charged atom, it is non-metal

16
Q

What is ionic bond

A

The bond formed between ions of opposite charge

17
Q

Properties of ions

A

Formed when atoms lose or gain one or more electrons
Group 1 metal gives 1 electron to the halogen if they react
Ions have the noble gas electronic structure with a complete outer shell
Giant ionic lattice structure

18
Q

When do ions conduct electricity and why

A

When melt or dissolved because the ions are free to move

19
Q

Boiling point and melting point of ions?

A

High BP and MP because the electrostatic force between ions are very strong

20
Q

Example of alloy

A

Brass - 70% copper, 30% zinc)

Harder than copper, does not corrode, used in musical instruments

21
Q

Define covalent bonding

A

When two non-metals share a pair of electrons to get full outer shells

22
Q

Define valency of an atom

A

The number of electron lost or gain to form a complete electron shell in a covalent or ionic compound

23
Q

Properties of covalent bonding

A

Covalent bonds within molecules are very strong

The forces between the separate molecules are weak - intermolecular force -> low melting point and boiling point

24
Q

Why do ionic compounds have high melting point and boiling point

A

Strong forces between the ion in the giant ionic lattice

25
Q

What is giant ionic lattice

A

Regular arrangement of alternating positive and negative ions

26
Q

Compare the volatility , solubility and electrical conductivity of ionic compounds and covalent compounds

A

Ionic - low volatility, usually soluble in water, conduct when molten or dissolved in water
Covalent - high volatility, insoluble in water, don’t conduct

27
Q

What is giant covalent structure

A

Network of covalent bonds through out the whole structure
Rigid 3D network of strong covalent bonds throughout the crystal so lots of energy to break the bond. They have high mp and bp

28
Q

Define allostropes

A

Different forms of the same element

29
Q

Describe the structure of diamond

A

A carbon atom forms 4 covalent bonds with other C atoms
Carbon atoms link together to form a giant lattice
High mp and bp
Very hard and cant be scratched easily -> use for cutting and drilling metal and glass
Does not conduct
Forms colorless glittering crystals -> use for jewellery

30
Q

Properties of graphite

A

Black and shiny solid
Carbon atoms are arranged in layers
Each C atom is joined to 3 other C atoms
Arranged in hexagon
Strong covalent bond within the layers=> a lot of energy is needed to break the bond -> high mp and bp
Bonding between layers is weak -> layers can slide over each other -> slippery feel and easily scratched
Weak bonding -> layers can flame off easily -> use as lubricant and in pencil
Conducts electricity

31
Q

Why does graphite conduct electricity?

A

Each C atom is bonded to 3 other C atom
C has 4 valency electrons
=> there are delocalized electrons move around along the layers
=> they drift along the layer when voltage is applied

32
Q

Properties of silicon(IV) dioxide

A

Makes up most of sand
Each silicon atom is bonded to 4 O atoms
Each Oxygen atom is bonded to 2 silicon atoms
Forms very hard colorless crystals -> high MP and BP
Does not conduct electricity bc it has no delocalized electrons

33
Q

What is metallic bonding?

A

Lattice of positive ions in a sea of electrons

34
Q

Why metal have high BP and MP?

A

It takes a lot of energy to weaken the strong force of attraction between the metal ions and delocalized electrons in the lattice

35
Q

Why metals are good conductor of heat and electricity

A

Delocalised electrons move through the metal lattice and carry energy through the metallic structure quickly
Conduction of heat is due to vibrations of the atoms passing on the energy form one atom to the next
The metallic structure allows the atoms to vibrate more freely

36
Q

Why are metals malleable and ductile?

A

Positive ions arranged regularly in layers so when force is applied, layers can slide over each other and new bond can easily form - this is because the attractive forces between the metal ions and the electrons act in any direction

37
Q

What is Ar?

A

Average mass of the atoms of an element, relative to thr mass of an atom of carbon 12

38
Q

What is Mr?

A

The sum of the relative atomic masses, call the relative molecular mass

Chemistry ✏️ (16 decks)

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