1.4: The Periodic table and patterns of change Flashcards by Madi H

How is the periodic table arranged as of 2014?

reading left to right, arranged in order of increasing atomic number.
7 horizontal period and 18 vertical groups

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What does the position of the elements mean?

Linked to physical and chemical properties, which allows for prediction

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What are vertical columns called?

groups

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What do the groups correspond to?

elements in the same group have similar chemical properties, they have the same amount of electrons in their outer shell

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What are group 1 elements called?

Alkali metals

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What do group 1 metals do in terms of reactions/reactivity?

They react with water to form hydrogen gas and an alkaline solution of the metal hydroxide.

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What happens to reactivity as you go down group 1?

they become more reactive

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What is the name of group 2?

Alkaline earth metals

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What happens to reactivity as you go down group 2?

they become more reactive

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What is the name of group 7/17?

halogens

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What is important about group 7?

they are the most reactive non-metallic group

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What happens to reactivity as you go down group 7?

reactivity decreases

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what is the name of group 0?

noble gases

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What happens to group 0?

They are inert/unreactive

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What are the horizontal rows called?

periods

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What do periods show?

The number of the period, gives the number of the highest occupied energy electron shell

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What blocks are present on the periodic table?

s, d, f, p (same as orbitals)

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What are elements that behave like both metals and non-metals called?

metalloids

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Why are group 2 called alkaline earth metals?

Because they form an alkaline solution with water

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What happens to group 2 in terms of atomic radius?
WHY?

It increases down the group
- number of electrons increases
- number of main electron shells increase
- more shielding to outermost electrons
- outer electrons repelled further from the nucleus

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What happens to group 2 in terms of Ionisation Energies?
WHY?

decreases down the group:
- atomic radius increases
- number of main electrons shells increase
- more shielding to outermost electrons
- weaker nuclear attraction to outermost electrons

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What happens to group 2 in terms of melting/boiling points?
WHY?

Decrease down the group:
- more shells and shielding
- weaker electrostatic attraction between positive cation
- less energy needed to overcome attraction

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What happens to group 2 in terms of reactivity?
WHY?

increases down the group
- will lose 2 e- which requires energy

outer electron (s) in shell further from nucleus
more shielding
weaker nuclear attraction
outer electron(s) more easily lost

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Metal + oxygen –>

metal oxide (basic oxide)

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Metal + oxygen --> example - magnesium

2Mg(s) + O₂(g) --> 2MgO (s)

Metal + oxygen --> What is observed when magnesium reacts?

Bright white flame for Mg, white solid oxides formed

Metal + oxygen --> example - calcium

2Ca(s) + O₂ --> 2CaO(s)

Metal + oxygen --> what is observed when calcium reacts?

Red flame for calcium, white solid oxides formed

Metal + water -->

Metal hydroxide + hydrogen

Metal + water --> example - magnesium

Mg(s) + 2H₂O(l) --> Mg(OH)₂ (aq) + H₂O PH - 8/9

Metal + water --> What is observed when magnesium reacts?

Very slow formation of bubbles of gas seen on the surface of magnesium

Metal + steam -->

Metal oxide + hydrogen (Mg only)

Metal + steam --> example - magnesium

Mg(s) + H₂O --> MgO (s) + H₂(g)

Metal + steam --> What is observed when magnesium reacts?

White solid formed

Metal + water --> example - calcium

Ca(s) + 2H₂O(l) --> Ca(OH)₂(aq) + H₂ PH - 10/11

Metal + water --> what is observed when calcium reacts?

Bubbles of gas and a white precipitate form

Metal + acid -->

metal salt + hydrogen

Metal + acid --> example: calcium + hydrochloric acid

Ca(s) + 2HCl (aq)--> CaCl₂(aq) + H₂(g) (calcium chloride + hydrogen)

Metal + acid --> magnesium + sulfuric acid

Mg(s) + H₂SO₄(aq) --> MgSO₄(aq) + H₂(g) Magnesium sulfate + hydrogen

Metal + acid --> Barium + nitric acid

Ba(NO₃)₂(aq) + H₂(g) Barium Nitrate + hydrogen

Metal + acid --> what observations are seen?

Bubbles of gas (effervescence), metal dissolves to form a colourless solution

Metal oxide + Water -->

Metal hydroxide (all group 2)

Metal oxide + Water --> example - Magnesium

MgO(s) + H₂O --> Mg(OH)₂ (aq) Magnesium hydroxide

Metal oxide + Water --> what is observed when magnesium reacts?

White solid dissolves

What molecules do halogens form?

Diatomic molecules

what kind of structure do halogens have and why?

The atoms are covalently bonded together so the halogens have a simple covalent structure

What happens to melting and boiling point as you go down group 2? WHY?

Melting and boiling point increase - More electrons - stronger London forces - more energy need to overcome attraction

What is the physical state of chlorine and fluorine at room temp?

gases

What is the physical state of bromine at room temp?

liquid

What is the physical state of iodine at room temp?

Solid

What kind of structure of halogens form?

simple molecular lattice

What happens to reactivity as you down group 7? WHY?

decreases - outer electron(s) in a shell further from nucleus - more shielding - weaker nuclear attraction - electrons less easily gained

What happens to the atomic radius of the atoms as you go across each period? WHY?

it get smaller - increasing number of protons - electrons are added to the same shell - no extra shielding - so a greater nuclear attraction for the outer shell of electrons to the nucleus - atomic radius decreases

How are melting and boiling point determined?

By the structure and bonding of the substance

What Melting and boiling points do giant structures have? WHY?

High - strong attractive forces between particles that must be broken - large amount of energy is therefore needed to break the bonds

What are giant structures?

Giant metallic / giant covalent

What Melting and boiling points do simple molecules and atoms have? WHY?

Relatively low - weak intermolecular forces between particles - forces depend on number of electrons - less energy is needed to overcome the intermolecular forces

Where are transition elements located on the periodic table?

with in the d-block (scandium through to zinc)

What is a d-block element?

An element with its outer electron in a d sub shell/orbital

What are transition metals?

An element that forms one or more stable ion which have a partially filled d-sub shell

What are the characteristics of transition metals?

- variable oxidation states - acts as catalysts - they form complex ions - they form coloured compounds

Using the table in your book learn the bold oxidation states!

Transition metals

What is the oxidation number of: Fe²+

What transition elements act as catalysts?

iron, platinum, palladium, rhodium, nickel

What is iron used for?

Making ammonia (haber process)

What is platinum, palladium, rhodium used for?

Catalytic converters

What is nickel used for?

Making margarine, hydrogenation of vegetable oils

What is a complex ion?

A central metal ion surrounded by ligands

What is a ligand?

A molecule or ion that donates a lone pair of electrons to the central metal ion to form a dative covalent (coordinate) bond

What is a coordination number?

The number of dative covalent bonds around the central metal ion

What is an example of ligands?

H₂O : Cl - : NH₃

What do all transition metals form when dissolved in water?

Hexaaqua ion

What is the formula for hexaaqua ion?

[X(H₂O)₆]²+

What is the formula for a hexaaqua Cooper (II) complex?

[Cu(H₂O)₆]²+

What is the Cooper ion surrounded by (in hexaaqua Cooper (II) complex)?

6 water ligands

What does the water molecule donate in the hexaaqua Cooper (II) complex. what does it form

Donates oxygen, to a lone pair of electrons to the central metal ions - forms a dative covalent/coordinate bond

What is the shape of the hexaaqua Cooper (II) complex?

Octahedral

What is the coordinate number in hexaaqua Cooper (II) complex? What is the bond angle?

6 90 degrees

What colour does copper ion form?

Blue solution

What is copper complex ion hexaaqua ion?

[Cu(H₂O)₆]²+

What colour does iron (II) form?

Pale green solution

What is iron (II) complex ion hexaaqua ion?

[Fe(H₂O)₆]²+

What colour does iron (III) form?

pale yellow solution

What is iron (III) complex ion hexaaqua ion?

[Fe(H₂O)₆]³+