Structure And Bonding Flashcards

1
Q

What are the 3 states of matter and their symbols

A

Solid(s) liquid (l) gas (g) aqueous (aq)

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2
Q

Describe the process of melting,

A

Solid turns into a liquid due to the heating of atoms inside, causing them to gain energy and vibrate and move freely until it overcomes the attractive forces

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3
Q

Describe the process of boiling

A

Liquid turns into a gas
Heating causes particles to move faster and collide increasing the vapor pressure until the liquid boils and forms gas bubbles

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4
Q

Describr the process of condensing

A

When a gas cools and loses energy causing its molecules to slow down and change into a liquid

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5
Q

What is the process of evaporation

A

When a liquid turns into a gas

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6
Q

What is the process of deposition

A

When a gas turns into a solid

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7
Q

Why do different substances have different melting and boiling points

A

Because the intermolecular forces between particles vary:

for example metallic compounds have giant structures, meaning they need more energy to break their many strong bonds, compared to other compounds that may have a weak intermolecular force between particles and therefore little energy needed to break it

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8
Q

Describe the factors that affect rate of evapotation

A

Temperature
Surface area
Structure of liquid (weak or strong bonds)
Air movement

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9
Q

State the particles involved in ionic bonding

A

(Positive) Metals and (negative) non metals

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10
Q

State the particles involved in covalent bonding

A

Non metal compounds

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11
Q

State the particles involved in metallic bonding

A

Metallic compounds

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12
Q

What are the properties of group 1 elements

A

Highly reactive - as they have a single electron on their outer shell which can easily become a +1 ion.

Low M and B point that decreases - there small number of electrons mean they have a weak structure, as you go down the molecules get larger and bonds become weaker

Good Conductors - their valence electron can move easily through the structure and carry a charge, therefore conduct

Reactivity increases as you go down - the outer electron gets further from the nucleus as you go down and can be lost more easily.

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13
Q

What are the properties of group 7 element

A

Don’t conduct - as there non metals

Highly reactive - 1 electron short of a full outer shell

M/B points are high that increase - have strong intermolecular forces, as you go down the atoms increase in size, as they gain extra electron shell which requires more energy to break

Reactivity decreases - As you move down the group, the atomic size increases, meaning that the outer electron is further from the nucleus. This results in a weaker attraction between the nucleus and the outer electron, making it harder for the halogen to gain an electron.

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14
Q

What are the properties of the noble gases

A

Poor reactivity - full outer shell

M and B points increases due to atomic sizes

Don’t conduct - they are monatomic (exist as individual atoms) and have a full valence shell, therefore no electrons to carry a charge

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15
Q

Describe how a group 1 metal atom becomes a positive ion

A

A Group 1 metal atom becomes a positive ion by losing its single outer electron, resulting in a positive charge. Because it only had 1 electron on its outer shell, it now has a full shell, (even if its zero)

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16
Q

What is an ion

A

A atom or molecule that has gained or lost an electron

17
Q

What is an iscotope

A

An atom of the same element with a different number of neutrons

Resulting in a different atomic mass

18
Q

Explain how electron transfer allows ionic bonding to occur in the compound formed when a group 1 metal reacts with a group 7 metal

A

Group 1 metals lose an electron and the group 7 nonmetals gain an electron. Leaving
Group 1s a positive charge and 7s a negative charge. These oppositely charged ions attracted to each other because of the electrostatic force, forming an ionic bond

19
Q

Explain the charge of a monatomic ion

A

The charge of a monatomic ion is determined by the number of electrons an atom gains or loses; if it loses electrons, it becomes a positively charged ion (cation), and if it gains electrons, it becomes a negatively charged ion (anion).

20
Q

Describe how a group 7 non-metal atom becomes a negative ion

A

Group 7 non-metals require 1 more electron to fill their outer shell, resulting in a negative charge as there are more electrons than protons

21
Q

Sublimation

A

When a solid turns into a gas