Ions & Bonding Flashcards by Maddie T

define atom

the smallest unit of matter that retains its properties

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what are the 3 subatomic particles?

protons, neutrons and electrons

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how is the mass number calculated?

number of protons + number of neutrons

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how is the number of neutrons calculated?

mass number - atomic number

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how is the atomic number calculated?

number of protons

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define isotopes

variations of the same element with different numbers of neutrons

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what subatomic particle affects the chemical properties of an element?

electrons

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do the physical properties change depending on the different isotopes of an element?

yes

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what physical properties vary between isotopes?

masses
densities
mpt / bpt

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how is the average mass of an element calculated?

isotope 1 (abundance x mass/ 100) + isotope 2 (abundance x mass/100)

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Define ion

charged atoms or molecules

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which is positive and which is negative; cations and anions

cations are positive and anions are negative

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Define bonding

the forces between particles that cause them to stick together

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Define structure

the 3D arrangement of particles as a consequence of bonding

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Define lattice

a repeating pattern of particles

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Define discrete

individual particles not arranged in a pattern

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Define allotropes

different structural forms of the same element (same chem. properties, different physical properties)

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Halogens exist as…

diatomic molecules held together by a single covalent bond

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What are the predicted properties of halogens?

low mpt (weak IMFs)
do not conduct
soluble only in oil-like substances

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What is the standard state color (aq) of:

F₂
Cl₂
Br₂
I₂

F₂ : (g) pale yellow (aq) colorless
Cl₂ : (g) pale green (aq) pale yellow
Br₂: (l) red/brown (aq) orange
I₂ : (s) grey (aq) brown/orange

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What is the relationship of mpt from F₂ - At₂

mpt inscreases from F₂ to At₂ because the particles get bigger and there is a larger surface area (more IMFs)

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Test 1 for halogens (damp blue litmus paper and starch)

Cl₂ damp blue litmus→red→white

Br₂ damp blue litmus→red→white
(slow)

I₂ starch→blue/black

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Test 2 for halogens (hexane test)

Cl₂ hexane→colorless

Br₂ hexane→orange

I₂ hexane→pink

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Cl₂ + H₂O→
Br₂ + H₂O→

HCl + HOCl
HBr + HOBr

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What color did the reaction of Fe and Cl₂ glow?

red

What happens to the mpt to alkaline earth metals (group 2)?

the mpt decreases but it is always higher than Group 1 due to the higher magnitude of charge and more delocalised electrons

What happens to the reactivity of Alkaline group metals (group 2)?

the reactivity increases but it is always lower than group 1 because they need to lose 2 electrons, not just 1

What are the 4 properties of transition metals?

- high mpt (higher than group 1 & 2) - high density - variable charges (2+,3+, → 8+) - form colored compounds

What are the colors of the following ions Fe²⁺ Fe³⁺ Cu²⁺ Mn²⁺ Mn⁷⁺ Cr³⁺ Cr⁶⁺

Fe²⁺.................green Fe³⁺.................orange/brown Cu²⁺.................blue Mn²⁺................pink Mn⁷⁺................purple Cr³⁺..................green Cr⁶⁺..................bright orange

Define inert

a full outer energy level which causes the atom to be unreactive

What are the properties of noble gases?

- very low mpt (weak inter-atomic forces) - do not conduct - insoluble in water - no bonding, exist as single atoms - full outer energy level

What are some of the uses for the following elements? He Ne Ar

He.............balloons / air-ships (less dense than air) Ne.............lighting (produces color with electricity) Ar..............light-bulbs (inert atmosphere)

What is electronic configuration?

(x,y,z)

How many energy levels do atoms have?

Why does the process of loss of electron require little energy?

1) electrons are located on the outside of an atom 2) electrons have small masses

How can the numbers of protons or neutrons be changed?

nuclear reactions

Why do atoms tend to lose or gain electrons?

to fully occupy their outer energy level

Where does ionic bonding occur?

in compounds containing a metal and a non-metal

GO MEMORISE THE TABLE MALU SENT TO YOU

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Define ionic bond

electrostatic force of attraction between oppositely charged ions

Why do ions attract in multiple directions?

because they are spheres (causes formation of a lattice)

Describe structure of NaCl

lattice of alternating cations and anions held together by electrostatic forces

Define properties

characteristics of chemicals

What are some properties that substances can have?

1) mpt / bpt 2) electrical conductivity 3) solubility 4) malleability

What does the strength of forces between particles depend on?

1) magnitude of charge 2) radius or ions (size)

Define electrical conductivity

charged particles that can move without breaking forces

In what states can ionic substances conduct?

liquid or aqueous

What are the 4 properties of ionic substances?

1) high mpt 2) conduct as (l) or (aq) 3) dissolve in water 4) brittle

What does malleability depend on?

forces present when particles move

Where does covalent bonding occur?

in substances containing 2 or more non-metals

How can covalent bonding be shown on a diagram?

bonding diagram or displayed formula

Define covalent bond

the electrostatic attraction of 2 nuclei for a shared pair of electrons

What are the 2 types of forces in a covalent discrete structure?

1) IMFs (weak) 2) covalent bonds (strong)

What are the 3 properties of covalent discretes?

1) very low mpt 2) do not conduct 3) only soluble in oil-like substances

Why do covalent discretes have a very low mpt?

because the IMFs are easy to break and mpt depends on the physical sie of the molecules

Why do covalent discretes not conduct?

because there are no charged particles

Why are covalent discretes only soluble in oil-like substances?

because during dissolving, molecules do not dissociate, the molecules only separate, meaning that only the IMFs need to be broken

What are the 4 properties of SiO₂ (sand)?

1) very high mpt 2) doesn't conduct 3) insoluble in all solvents 4) brittle

Describe the structure of SiO₂

lattice of atoms held together by strong covalent bonds, not IMFs

Pick the correct word to fill in the blanks: words:【only one force/both forces】 Most covalent structures have ________________, covalent and/or discrete

only one force

What are the 3 properties of diamond?

1) very high mpt (~3500 Cº) 2) does not conduct 3) does not dissolve in any solvent

What are the only 3 covalent substances to have a lattice structure?

1) SiO₂ 2) C in diamond 3) C in graphite

What are the properties of graphite?

1) high mpt 2) conducts electricity due to delocalised electrons 3) insoluble in every solvent 4) lubricant, layers can slide over each other without affecting the rest of structure

Where does metallic bonding occur?

metallic elements

Describe a metallic element

a lattice of cations surrounded by delocalised electrons held together by strong electrostatic forces

What are the 4 characteristics of metallic elements?

1) high mpt 2) conduct 3) insoluble in all solvents 4) malleable

What is the relationship with color from F₂→At₂?

color becomes darker

What is the relationship of alkali group 1 metals when moving down with mpt?

decreases

What is the relationship of halogens group 2 non-metals when moving down with mpt?

increases

What is the relationship of alkali group 1 metals when moving down with reactivity?

increases

nvm