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Flashcards in chemistry Deck (46):
1

explain how the electron structure of an atom determines its properties

- how readily they accept or donate an electron,
- determines how they bond with nearby elements(strength and physical characteristics) and
- how many free electrons they donate (conductivity)

2

Explain how the chemical properties of an element help to determine its position in the periodic table.

by the atomic number as they are in ascending order,
- the reactivity decreases as you go from left to right,
- ionisation increases from left to right

3

Outline the development of the modern Periodic Table.

the number of protons determine where it is on the periodic table

4

Understand why elements in the same group of the Periodic Table have similar properties

because they have the same number of electrons in their valance shell

5

Identify the location of metals, metalloids and non-metals on the Periodic Table

metals are on the left, metalloids are in the middle and non-metals are on the right

6

name the groups

Group 1 alkali metals,
Group 2 alkaline earth metals,
Groups 3-12 transition metals,
Group 17 halogens
Group 18 noble gases.

7

Use models and diagrams to describe the nature of the bonding in metallic solids

sea of electrons moving as the element stays put

8

Use models and diagrams to describe the nature of the bonding in ionic solids

lattice structure
- metal with the valance electron next to it

9

Use models and diagrams to describe the nature of the bonding in covalent solids

sharing of electrons, joining two elements together

10

Distinguish between covalent molecular and covalent network solids.

covalent network: between multiple atoms forming a big structure
covalent molecular: only between a few atoms

11

properties of metallic

metallic: high melting and boiling points, insoluble

12

properties of ionic

high melting and boiling point,
many dissolve,
do not conduct electricity as solids only as liquids,
positive and negative ions strongly attracted together

13

properties of covalent molecular

strong covalent bonds,
weak intermolecular forces,
low melting and boiling points
do not conduct electricity,
neutral

14

properties of covalent networks

strong covalent bonds throughout the whole structure,
high melting and boiling points,
do not conduct electricity,
no moving charges

15

element

a substance composed of atoms

16

atom

particles that make up all material, take part in reactions

17

nucleus

core of the atom, made of protons and neutrons

18

proton

positively charged particle found in the nucleus

19

neutron

neutrally charged particle found in the nucleus

20

electron

negatively charged particle found in the shells

21

ion

positive or negative charged atom or group of atoms

22

isotope

atoms of the same element with a different number of neutrons

23

atomic number

the number of protons or electrons in an atom

24

mass number

number of protons and neutrons in the nucleus

25

energy shell

regions surrounding the nucleus, where electrons are found

26

valance shell

the outer most shell

27

electron configuration

number of electrons in each shell

28

group

vertical columns on the periodic table

29

periods

horizontal rows on the periodic table

30

cation

positively charged ion

31

anion

negatively charged ion

32

ionic

substance made or positive and negative ions

33

relative atomic mass

the mass of an atom compared with 1/12th of a carbon 12 atom

- the mass number
- no grams or gmol

34

molar mass

same as relative atomic mass but with gmol-1
- atomic mass

35

relative molar mass

the molar mass of a covalent molecule (two or more atoms)

36

relative formula mass

molar mass of a covalent network or a ionic lattice

37

mole

6.02x10^23

38

ionic bond

metal + non-metal

39

covalent bond

non-metal + non-metal

40

metallic bond

metal + metal

41

if ..ide how do you work it out

same as the periodic table

42

what is m

mass g

43

what is n

the number of moles

44

what is M

molecular mass
- the mass number
- gmol-1

45

converting from mass to moles

mass divided by the mass number

46

converting from moles to mass

multiply the number of moles by the mass number