Atomic Structure and Bonding

Question 1

What does the octet rule refer to?

Answer 1

the tendancy of atoms to prefer to have 8 electrons in their outer shell

Question 2

Valence shell electrons

Answer 2

electrons which are lost or gained to form ions

Question 3

What charge does a nucleus have?

Answer 3

positive

Question 4

describe ionic compounds

Answer 4

ionic compounds are formed during a reaction between a metal atom and a non-metal atom. The metal atom loses electrons, forming positively charged ions called cations.
The non-metal atom gains electrons, forming negative ions called anions.
The ions are held together by the strong lectrostatic force of attraction of the oppositely charged atoms.

Question 5

What is an ionic bond?

Answer 5

Electrostatic force of attraction between oppositely charged ions

Question 6

What is a lattice

Answer 6

Regular repeated 3-D arrangement

Question 7

What does Giant refer to in Giant Ionic Lattice?

Answer 7

unlimited amount of ions, can’t state how many irons there is

Question 8

Polyatomic meaning

Answer 8

composed of two or more atoms covalently bonded

Question 9

describe what happens when lithium chloride forms in terms of e- transfer (5)

Answer 9

-lithium loses one electron
-Chlorine gains one electron
-Lithium has a positive charge
-Chlorine has a negative charge
-Electrostatic force of attraction between opposite charges

Question 10

non metal and metal bonding??

Answer 10

ionic bonding

Question 11

Why do ionic compounds have high melting and boiling points?

Answer 11

It is a giant ionic structure and the strong electrostatic force of attraction between ions require a lot of heat energy to break

Question 12

why are ionic compound soluble in water?

Answer 12

Water molecules are able to break the electrostatic force of attraction between ions, because water is polar

Question 13

Why don’t ionic, solids, conduct, electricity

Answer 13

because it is a fixed structure and Ions aren’t free to move or carry charge

Question 14

why can ionic liquids conduct electricity?

Answer 14

Ions can move past each other and charge can flow making an electric current

Question 15

What does brittle mean?

Answer 15

when a force is applied, ions in lattice shift so that like ions repel and lattice breaks

Question 16

why ionic compounds hard?

Answer 16

Because of the strong, electrostatic force of attraction between oppositely charged ions

Question 17

AMMONIUM TEST

Answer 17

add dilute sodium hydroxide (NaOH) solution
- gently heat
- if NH4 is present, a pungent smell, identified using damp, red litmus paper held above test tube

Question 18

CARBONATE TEST

Answer 18

add dilute hydrochloric acid
Bubble gas through limewater
If present, limewater will turn cloudy

Question 19

SULFATE TEST

Answer 19

add dilute hydrochloric acid
Add drops of barium chloride
Is present a white precipitate will form

Question 20

HALIDE ION TEST

Answer 20

add dilute nitric acid
Add drops of silver nitrate solution
If it’s Cl, white precipitate
If it’s Br, cream precipitate
If it’s I, a yellow precipitate

Question 21

What is a test used for Li, Na, K or Ca?

Answer 21

Flame test

Question 22

FLAME TEST RESULTS

Answer 22

red- lithium
yellowey orange- sodium
purple- potassium
brick red- calcium

Question 23

what is a precipitate?

Answer 23

An insoluble solid formed from 2 soluble solutions

Question 24

what are the general properties of metals?

Answer 24

high melting and boiling points
Good conductors of heat and electricity
Hard
Malleable
Ductile

Question 25

Describe metallic bonding

Answer 25

lattice of metal cations are attracted to the sea of the delocalised valence shell electrons. This electrostatic force of attraction is called metallic bonding.

Question 26

What name is given to structure that simple covalent compounds form?

Answer 26

molecule

Question 27

Characteristics of a simple covalent bond

Answer 27

Low melting and boiling points, not electrically conductive exhibit weak intermolecular forces not soluble in water

Question 28

Giant covalent bond characteristics

Answer 28

high melting and boiling points Not electrically conductive Exhibit strong covalent, bonding Not soluble in water

Question 29

Why can metals conduct electricity?

Answer 29

delocalised valence shell electrons can move through the structure and carry charge

Question 30

Why can metals conduct heat?

Answer 30

delocalised valence shell electrons can move fastly and pass energy on quickly the lattice of electrons transmits energy efficiently, as atoms vibrate and bump into other atoms

Question 31

Why do metals have high melting and boiling points?

Answer 31

electrostatic forces of attraction between delocalised valence electrons and cations are strong and require a lot of heat energy to break them

Question 32

why are metals malleable?

Answer 32

Arrangement of atoms change, but the attraction between delocalised balance of electrons and cations isn’t broken

Question 33

Metallic bond characteristic

Answer 33

high melting and boiling point Electrically conductive Hard malleable Not soluble in water

Question 34

Alloy

Answer 34

combination of two or more metals

Question 35

Alloy characteristics

Answer 35

harder than pure metals Less malleable than pure metals poorer conductors than pure metals

Question 36

covalent bonding

Answer 36

Electrostatic force of attraction between the nuclei of two atoms and shared pairs of electrons between them

Question 37

Covalent bond

Answer 37

Chemical bond that involves the sharing of valence electron pairs between atoms forming between non-metal elements. Very strong bonds

Question 38

polarity

Answer 38

Nucleus has pull on electrons. Strength of pull depends on atom. UNEVEN DISTRUBUTION OF CHARGE ACROSS A MOLECULE

Question 39

Giant covalent structures

Answer 39

many atoms join to adjacent atoms by covalent bonds. Arranged into giant ionic lattices extremely strong structures because of many bonds

Question 40

simple, covalent molecules consist of a small number of atoms bonded together through ________ _____

Answer 40

covalent bonds

Question 41

Allotrope, with example

Answer 41

different forms of the same element in the same state. Eh, Graphite, Diamond

Question 42

why do giant covalent substances have high melting and boiling points?

Answer 42

A lot of simple covalent bonds requiring high temperatures to melt or break.