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Chemistry > Module 2 > Flashcards

Module 2 Flashcards

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1
Q

orbital

A

a region that can hold u to 2 electrons of opposite spins

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2
Q

ionic bonding

A

strong electrostatic attraction between oppositely charged ions

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3
Q

covalent bonding

A

shared pair of electrons

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4
Q

dative covalent bonding/coordinate bonding

A

the shared pair of electrons where both electrons come from the same atom

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5
Q

metallic bonding

A

electrostatic attractions between positive metal ions and negative delocalised electrons

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6
Q

electronegativity

A

the ability of an atom to attract the bonding electrons in a covalent bond

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7
Q

permanent dipole-dipole force

A

intermolecular forces that exist because of the difference in electronegativities in a polar bond causes week electrostatic forces of attraction between molecules

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8
Q

acid

A

proton donor

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9
Q

strong acid

A

acid that completely dissociates in water

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10
Q

weak acid

A

acid that partially dissociates in water

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11
Q

base

A

proton acceptor

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12
Q

alkali

A

releases OH- ions into solution

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13
Q

salt

A

when a H+ in an acid is replaced by a metal ion or an ammonium ion

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14
Q

concordant results

A

titre values that are within 0.1cm3 of each other

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15
Q

oxidising agent

A

a substance that is reduced in a redox reaction

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16
Q

reducing agent

A

a substance that is oxidised in a redox reaction

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17
Q

empirical formula

A

the simplest whole number ratio of atoms present in a compound

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18
Q

molecular formula

A

the actual number of atoms of each element in a molecule

19
Q

hydrated salts

A

contains water of crystallisation

20
Q

anhydrous salts

A

contains no water of crystallisation

21
Q

isotopes of the same element have:

A

-the same number of protons and electrons
-a different number of neutrons

22
Q

what are the properties of isotopes

A

-they have the same chemical properties
-as they have the same number of electrons

23
Q

relative atomic mass

A

the average mass of an atom relative to 1/12th the mass of one atom of C12

24
Q

relative isotopic mass

A

the mass of isotopes compared to 1/12th the mass of one atom of 12C

25
Q

between what elements is covalent bonding

A

non-metals

26
Q

between what elements is ionic bonding

A

a metal and non metal

27
Q

what are the anomalies of the octet rule

A

-boron and beryllium are stable with only 6 electrons in their outer shell
-sulfer can hold 12 electrons in it’s outer shell

28
Q

what shape and angle is the shape when the central atom has 2 bonding a pairs and 0 lone pairs

A

-linear
-180

29
Q

what shape and angle is the shape when the central atom has 3 bonding pairs and 0 lone pairs

A

-trigonal planar
-120

30
Q

what shape and angle is the shape when the central atom has 4 bonding pairs and 0 lone pairs

A

-tetrahedral
-109.5

31
Q

what shape and angle is the shape when the central atom has 3 bonding pairs and 1 lone pair

A

-trigonal pyramidal
-107

32
Q

what shape and angle is the shape when the central atom has 6 bonding pairs and 0 lone pairs

A

-octahedral
-90

33
Q

what shape and angle is the shape when the central atom has 2 bonding pairs and 2 lone pairs

A

-non linear
-104.5

34
Q

what shape and angle is the shape when the central atom has 2 regions of electron density

A

-linear
-180

35
Q

how to explain bond angles and shapes in the exam

A

-state the angle and shape
-there are _ bonding pairs and _ lone pairs around the _ atom
-all electron pairs repel each other and get as far away as possible from each other
-lone pairs of electrons repel more strongly than bonding pairs of electrons

36
Q

what is a polar bond

A

-when there is a difference in electronegativity

37
Q

what is a non polar bond

A

-when there is no difference in electronegativity
-carbon bond to hydrogen is classed as non polar as the difference in electronegativity is very small

38
Q

dipole

A

partial positive and negative charge caused by the uneven distribution of electrons

39
Q

what causes a permanent dipole

A

-the difference in electronegativity between two atoms

40
Q

how do induced idol-dipole interactions/london forces occur

A

-caused by the movement of electrons within shells
-this causes an instantaneous dipole across the molecule
-this instantaneous dipole in one molecule induces a dipole on a neighbouring molecule which then induces a dipole on their neighbouring olecule
-the small induced dipoles attract each other causing a weak intermolecular force

41
Q

ionic compounds structure, melting and boiling points

A

-have a giant ionic structure
-very high melting and boiling pints
-have strong electrostatic attraction between oppositely charged ion
-require lots of energy to overcome

42
Q

ionic compounds - solubility

A

-soluble in water as water is polar
-water molecules pull the ions away from the lattice causing it to dissolve

43
Q

ionic compounds - conductivity

A

-conducts electricity when molten or dissolved as ions are mobile
-can’t conduct when solid are ions are in a fixed position

44
Q

metallic compounds structure, melting and boiling points

A

-giant metallic lattice
-very high melting and boiling points
-as have very strong metallic bonds
-need lots of energy to overcome

Chemistry (9 decks)

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