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Flashcards in 1 - Periodic Table Deck (46)
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1

Relative Isotopic Mass?

Is the mass of an isotope, relative to 1/12 of the mass of an atom of carbon -12

2

Relative atomic mass?

Is the weighted mean mass of an atom of an element, relative to 1/12 of the mass of an atom of carbon 12

3

How is an ion formed?

By the loss or gaining of electrons

4

Relative charge of a proton?

+1

5

Relative charge of a neutron?

0

6

Relative charge of an electron?

-1

7

What is the mass number?

The biggest number, contains protons and neutrons

8

What is the proton number?

number of protons + electrons

9

Calculating relative atomic mass

75.78 % of chlorine -35
24.22% of chlorine -37

75.78 x 35 + 24.22 x 37 / 100

10

Calculating moles?

How many moles of phosphorus pentoxide (P4O10) are in 85.2g?
P= 31
O=16
31x4 +16x10 = 284

85.2 / 284 = 0.3 moles

11

Relative molecular mass?

N2 = 14 x 2 = 28

12

Relative atomic mass?

Copper: 120.8% = 63
54% = 65

120.8 x 63 + 54 x 65/ 174.8
= 63.6

13

Stages of mass spectrometry?

Gas injected in ionizer with electrons.
Beam of electrons is bombarded at electrons and sample is ionized.
Ions are accelerated in an electric field.
Then bend through magnetic field.
Deflected by electric field.

14

What is the vacuum for in a mass spectrometer?

Means there's no interference from other ions.
High energy electrons are used to make the positive ion

15

Flame test: sodium chloride?

Yellow/ orange

16

Flame test: Lithium chloride?

red/ pink

17

Flame test: Calcium chloride?

yellow/ orange

18

Flame test: Barium chloride?

green

19

Flame test: Copper chloride?

Green/blue

20

Flame test: Potassium chloride?

lilac/ pink

21

Emission spectra?

If an electron takes in energy from its surroundings it's excited to a higher energy level. When they drop to a lower energy level, they release this energy. (this is what we observe)

22

how many electrons does the S orbital hold?

2 electrons

23

How many electrons does the P orbital hold?

6 electrons

24

How many electrons does the D orbital hold?

10 electrons

25

How many electrons does the F orbital hold?

14 electrons

26

First 7 electronic configuration?

1s2s2p3s3p4s3d

27

Electronic configuration of Argon? 18 electrons

1s2, 2s2, 2p6, 3s2, 3p6

28

Using the noble gas in the above row to shorten electronic configuration

Scandium 21 Argon = 18
(Ar) 3s2, 3p1

29

Hunds rule?

Electrons will occupy the orbitals singularly before pairing takes place.

30

Pauli's exclusion principle?

2 electrons cannot occupy the same orbital, unless they have opposite spins.