Brainscape's Knowledge GenomeTM

Browse over 1 million classes created by top students, professors, publishers, and experts.


See full index

Year 10 Chemistry > Chemical Formulas And Bonding > Flashcards

Chemical Formulas And Bonding Flashcards

1
Q

What is a molecular formula?

A

This refers to the representation of a molecule using chemical symbols to indicate the type of atom and subscripts to indicate the number of atoms of each type present in the molecule

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
2
Q

Name the 3 types of chemical formulas

A

a. Molecular formula
b. Structural formula
c. Empirical formula

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q

What is the structural formula?

A

This is the type of formula which shows how atoms are connected in a molecule

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
4
Q

What is a chemical bond?

A

This is the force of attraction that exists between atoms or ions holds them together in a crystal or molecule.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
5
Q

Give 2 examples of a molecular formula

A

CH4
H2O

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
6
Q

What is the difference between a ball-and-stick model and a space-filling model?

A

A ball and stick model shoes the geometric arrangement of the atoms with respective atomic sizes
whereas
space-filling model shoes the relative sizes of the atoms

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
7
Q

Define empirical formula

A

This indicates the type of atoms present and the simplest whole number ration of the number of atoms in the compound

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
8
Q

Give an example of an empirical formula

A

Titanium dioxide -TiO2

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
9
Q

Molecules of glucose contain 6 carbon atoms, 12 hydrogen atoms and 6 oxygen atoms. What are the molecular and empirical formula of glucose?

A

Molecular- C6H12O6
Empirical- CH2O

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

Define isomers

A

Isomers are compounds with the same chemical formula but different molecular structure

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
11
Q

Name the types of isomers

A

a. Spatial isomers
b. Structural isomers

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
12
Q

Define the types of isomers

A
  1. Structural isomers - these are isomers with the same chemical formula but doff structure and therefore different chemical properties
  2. Spatial isomers - these are isomers that their relative orientations of the atoms in space differ
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
13
Q

An ion found in some compounds used as antiperspirants contains 13 protons and 10 electrons. What is its
symbol?

A

Because the number of protons remains unchanged when an atom forms an ion, the atomic number of the
element must be 13. Knowing this lets us use the periodic table to identify the element as Al (aluminum).
The Al atom has lost three electrons and thus has three more positive charges (13) than it has electrons (10).
This is the aluminum cation, , Al3+

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
14
Q

Aluminum and carbon react to form an ionic compound. Predict which forms an anion, which forms a
cation, and the charges of each ion. Write the symbol for each ion and name them.

A

Answer: Al will form a cation with a charge of 3+: Al3+, an aluminum ion. Carbon will form an anion with
a charge of 4−: C4−, a carbide ion

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
15
Q

What are monoatomic ions?

A

These are ions formed from only one atom

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
16
Q

What are oxyanions?

A

These are polyatomic ions that contain one or more oxygen atoms

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
17
Q

What are ionic bonds?

A

These are the electrostatic forces of attraction that exist between particles of opposite charges

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
18
Q

What is another name for ionic bonds?

A

Electrostatic bonds

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
19
Q

What are covalent bonds?

A

A covalent bond is a bond formed by sharing of electrons between atoms in which each atom contributes an electron .

20
Q

Another name for covalent bonds is…

A

Molecular bonds

21
Q

Define ionic compounds

A

These are compounds formed as a result of the complete transfer of one or more electrons from a metal to a non-metal.

22
Q

What 2 techniques help to determine molecular formulas?

A

a. Qualitative analysis
b. Quantitative analysis

23
Q

Define the 2 techniques used to determine molecular formulas

A

a.Quantitative analysis is a type of analysis which determines the mass, especially the percentage by mass of the different elements present in a compound.

b.Qualitative analysis is a type of analysis which determines the different type of element, ions or functional groups present in a compound/species.

24
Q

What 3 ways can structural formulas be expressed in?

A

I. Condensed structural formula
II. Dashed/Display structural formula
III. Skeletal structural formula

25
Q

Give 4 properties of ionic compounds

A

a. Conducts electricity in the molten state not solid state
b. Has high melting, boiling and freezing points
c. Electrically neutral
d. Soluble in polar solvents but insoluble in non-polar solvents

26
Q

Predict the formula of the ionic compound formed between the sodium cation, Na+
, and the sulfide anion,
S2-

A

Na2S

Why?
Because an ionic compound must be electronically neutral and since sodium has one cation but sulphide has 2 anions, there has to be 2 sodium atoms to react with the sulphide anion for the formula to be neutral

27
Q

What are the two main types of chemical bonds?

A

The two main types of chemical bonds are interatomic bonds (intramolecular bonds) and intermolecular bonds.

28
Q

Define interatomic bonds.

A

Interatomic bonds are forces that hold atoms together in a molecule, including ionic, metallic, and covalent bonds.

29
Q

What are the two main types of intermolecular bonds?

A

The two main types of intermolecular bonds are hydrogen bonding and Van der Waals forces.

30
Q

What is the Lewis structure?

A

The Lewis structure is a diagrammatic representation of elements or compounds using valence electrons, proposed by G.N Lewis.

Lewis Structure is a very simplified representation of the valence shell electrons in a molecule.

31
Q

What is the Octet Rule?

A

The Octet Rule states that atoms share electrons with neighboring atoms to achieve a noble gas configuration of 8 or 2 valence electrons.

32
Q

Give examples of exceptions to the Octet Rule.

A

Exceptions to the Octet Rule include species with odd numbers of electrons (e.g., NO and NO2), incomplete octets (e.g., BeCl2), and expanded octets (e.g., SF6).

33
Q

Describe an ionic bond.

A

An ionic bond is the electrostatic force of attraction between a cation and anion formed by the transfer of electron(s) from an atom of low ionization energy to another atom of high electron affinity.

34
Q

What are the factors that influence the formation of an ionic compound?

A

The factors that influence the formation of an ionic compound are low ionization energy of the metal, high electron affinity of the non-metal, and high electronegativity difference between the atoms involved (equal or greater than 1.7).

35
Q

List three properties of ionic compounds.

A

Three properties of ionic compounds are: they are crystalline solids, they are hard and brittle, and they have high melting points and high boiling points.

36
Q

Define metallic bonding.

A

Metallic bonding is the electrostatic force of attraction between the delocalized electrons and fixed positive metal ions.

37
Q

What are two factors that affect metallic bonding?

A

The number of valence electrons and atomic size are two factors that affect metallic bonding.

38
Q

Describe a covalent bond.

A

A covalent bond is a bond formed by sharing of electron pair between atoms in which each atom contributes an electron.

39
Q

What are the unique material properties of metals due to metallic bonding?

A

The unique material properties of metals due to metallic bonding include excellent thermal and electrical conductivity, high melting points, and malleability.

40
Q

Do ionic compounds conduct electricity in molten form or in an aqueous state?

A

Ionic compounds conduct electricity in molten form or in an aqueous state, but not in solid form.

41
Q

Describe a pure or non-polar covalent bond.

A

A pure or non-polar covalent bond is formed when the shared pair of electrons is equally shared between the atoms because the two atoms have the same electronegativities.

42
Q

What are some examples of covalent compounds?

A

Examples of covalent compounds include H2, N2, Cl2, O2, H2 (formed between the same atoms), CH4, HCl, HBr, CO, NH3 (formed between different atoms), and silica, diamond, graphite (giant molecules).

43
Q

Define a polar covalent bond.

A

A polar covalent bond is formed when there is unequal sharing of electron pair between two atoms due to a difference in electronegativities.

44
Q

How is a dative or coordinate covalent bond formed?

A

A dative or coordinate covalent bond is formed when one species donates a lone pair of electrons to another species that has an empty orbital to accept the electrons.

45
Q

What factors favor the formation of covalent bonds?

A

Factors that favor covalent bond formation include high electron affinity of the bonding atoms, high ionization energy of the bonding atoms, and low electronegativity difference between the two bonded atoms.

46
Q

Describe the properties of covalent compounds.

A

Covalent compounds usually exist as gases and liquids at room temperature, have low melting and boiling points, do not conduct electricity except for graphite, and dissolve in non-polar solvents but not in polar solvents.

Year 10 Chemistry (6 decks)

Brainscape helps you reach your goals faster, through stronger study habits.
© 2024 Bold Learning Solutions. Terms and Conditions