Chapter 2

Question 1

How thingd measured in mass relatively? (DONT NEED TO KNOW)

Also what happened that means we can’t just measure the masses of protons electrons neutrons?

Answer 1

• standard isotope on which all atomic masses will be relative to is chosen as carbon 12
• Mass carbon 12 isotope is defined as exactly 12 atomic units (U)
• standard unit is one U which is 1/12th
• thus is roughly same mass as portion / neutron

2) mass defect, nucleus binds holding nucleus comes with a small decrease of mass (Einstein ) (don’t need to know)

Question 2

Isotope definition

Answer 2

Atoms of the same elements with different number of neutrons and different masses

(Sam’s protons, different mass number due to different amount of neutrons)

Question 3

Relative isotopic. Mass

Answer 3

Mass of an isotope relative with 1/12 of the mass of an atom of carbon 12

(Can assume it’s same as mass number if they don’t give )

Question 4

Relative atomic mass

Answer 4

Weighted mean mass of an atoms of an element relative to the 1/12th of the mass an atom of carbon 12

Question 5

Mass spectrometry

Answer 5

A

Question 6

What does it mean by weighted mean mass (as part of relative atomic mass)

Answer 6

Weighted mean mass takes account if

• percentage abundance of Esch isotope
• the relative isotopic mass of each isotope

As in multiply abundance by each isotopic mass then divide by hundred, takes in account of these

Question 7

What is mass spectrometry used for

2 Pints

Answer 7

• 1. determination of relative isotopic masses and relative abundances of each isotope (so Esch mass and then how abundant it is and then
     
     2. calculation of relative atomic mass of an element from the relative abundance of its isotope

(All of the masses and their abundsncies are avaegrad out based on percentages to make relative atomic mass)

Question 8

How to work relative atomic mass by hand

Answer 8

Multiply each mass by the percentage (M/ RSTIO ON HRAPH)

Add

Divide by hundred

Question 9

What is m/z (kinda important)

Answer 9

If charge of ion is plus 1, m/z is same mass of ion which is same mass of element too

Question 10

Atom

What do a and z represent

Deuterium ?

Answer 10

• nucleus protons neutrons, electrons in shells
• electron 1/1836 mass of proton
• neutrons is glue between atom holding the nucleus together a s protons repel (waffle)
• z number of protons , a protons and neutrons
  3) deuterium is just 2/1 hydrogen, with a neutron, and heavy water is D2O. As more heavy isotope boiling melting density increase

Question 11

Isotopes change Physical but not chemical reactions how?

Answer 11

Chemical reactions depend on electrons surrounding nucleus, but electrons are constant

Higher mass isotopes will have higher melting boiling snd density tho

Question 12

Charge on Zn and Ag

Answer 12

Zn+2 , Ag+1

Question 13

Binary compund

Answer 13

Contains two elements only

Question 14

Polyatomic SHANC

Answer 14

Sulfate SO4 2-
Hydorixide OH-
Amomminum NH4+
Nitrate = No3 -
Carbonate = CO3-2

4 are sulfate and ammonium

Question 15

Nitrite sulfide?

Answer 15

Same charge one less oxygen due to “ite”

= NO2-
= SO3-2

Question 16

Hydrogen carbonate

Answer 16

HCO3-

Carbonate = co3-2, h= + so combine

Question 17

Manganite (7)permanganate

Answer 17

MnO4-

Question 18

Dichromate

Answer 18

CR2O7 -2 Uday

Question 19

Phosphate

Answer 19

PO4 - 3

Question 20

Phosphors and sulfur?

Answer 20

P4 and S8, but sulfur can be normal S

Question 21

What becomes aqueous ?

Answer 21

Acids,

Alkalis with OH , bases, rest with carbonate and oxide etc

Question 22

CHEMICAL PROTPETIES

Answer 22

Determined by amount of electrons in OUTER DHELL INLY