Unit 1 Test

Question 1

When does the chemical reactivity of a metal decrease?

Answer 1

When you go across a period.

Question 2

When does the chemical reactivity of a metal increase?

Answer 2

As you go down a group of metals

Question 3

What is ionization energy?

Answer 3

The energy required to remove the most loosely bound electron from a gaseous atom or ion.

Question 4

What is the second ionization energy?

Answer 4

the energy required to remove the second most loosely bound electron from a gaseous atom or ion.

Question 5

When does ionization energy decrease?

Answer 5

As you go down a group.

Question 6

When does ionization energy increase?

Answer 6

When you go across a period.

Question 7

What is a screening electron?

Answer 7

The electrons that are found in the inner orbits between the nucleus and the valence electrons.

Question 8

When does atomic radius increase?

Answer 8

Down a group.

Question 9

When does atomic radius decrease?

Answer 9

Across a period.

Question 10

When does electron affinity increase?

Answer 10

Across a period.

Question 11

When does electron affinity decrease?

Answer 11

down a group.

Question 12

When does electronegativity increase?

Answer 12

across a period.

Question 13

When does electronegativity decrease?

Answer 13

down a group.

Question 14

When does the reactivity of non-metals increase?

Answer 14

across a period.

Question 15

When does the reactivity of non-metals decrease?

Answer 15

down a group.

Question 16

When does a non-polar covalent bond occur?

Answer 16

If the difference in electronegativity is 0.5 or less (the electron sharing is EQUAL)

Question 17

When does a polar covalent bond occur?

Answer 17

When the difference in electronegativity is between 0.5 and 1.7 (the electron sharing is UNEQUAL)

Question 18

When do ionic bonds generally occur?

Answer 18

In ionic compounds; generally occurs between metal and nonmetal atoms where the difference in electronegativity is greater than 1.7.

Question 19

What happens in an ionic bond?

Answer 19

The nonmetal atom will pull valence electrons away from the metal atom due to a greater electronegativity value. Electron transfer occurs, sharing does not take place

Question 20

What is electron affinity?

Answer 20

An atom’s ability to attract electrons.

Question 21

What is atomic radius?

Answer 21

The distance from an atom’s nucleus to its outermost electron.

Question 22

What is electronegativity?

Answer 22

A term which is used to represent the relative attracting power of an atom for a pair of bonding electrons.

Question 23

Why is the second ionization energy greater than the first ionization energy?

Answer 23

Because the electron is being removed from a positive ion rather than from an atom, which will require more energy.

Question 24

ionic compounds: what particles are involved in the bond?

Answer 24

oppositely charged ions

Question 25

ionic compounds: what type of bonding?

Answer 25

ionic

Question 26

ionic compounds: what state at room temperature?

Answer 26

crystalline solids

Question 27

ionic compounds: what is the melting point?

Answer 27

high

Question 28

ionic compounds: what is the solubility in water?

Answer 28

most have high solubility

Question 29

ionic compounds: do they have electrical conductivity as a liquid?

Answer 29

yes

Question 30

ionic compounds: do they have electrical conductivity when dissolved in water?

Answer 30

yes

Question 32

molecular compounds: what particles are involved in the bond?

Answer 32

molecules

Question 33

molecular compounds: what type of bonding?

Answer 33

covalent

Question 34

molecular compounds: what state at room temperature?

Answer 34

solid, liquid or gas

Question 35

molecular compounds: what is the melting point?

Answer 35

low

Question 36

molecular compounds: what is the solubility in water?

Answer 36

most have low solubility

Question 37

molecular compounds: do they have electrical conductivity as a liquid?

Answer 37

no

Question 38

molecular compounds: do they have electrical conductivity when dissolved in water?

Answer 38

not usually

Question 39

what is the latin nomenclature name for iron?

Answer 39

ferrum.

Question 40

what is the latin nomenclature name for tin?

Answer 40

stannum

Question 41

what is the latin nomenclature name for lead?

Answer 41

plumbum

Question 42

what is the latin nomenclature name for copper?

Answer 42

cuprum

Question 43

Define science.

Answer 43

A highly logical, systematic and organized approach to problem solving.

Question 44

define ion

Answer 44

a charged particle

Question 45

define compound

Answer 45

a pure substance which is made up of 2 or more different types of elements.

Question 46

define atomic number.

Answer 46

corresponds to the number of protons or electrons present in a single atom

Question 47

define relative mass

Answer 47

the average atomic mass of an element.

Question 48

define the octet rule.

Answer 48

atoms react chemically to achieve a noble (inert) gas electron arrangement.

Question 49

define chemistry.

Answer 49

a science which studies substances, their properties, structure, composition, and transformations.

Question 50

define molecules.

Answer 50

larger particles that are created when atoms join together.

Question 51

what is a pure substance?

Answer 51

a form of matter which is made up of only 1 kind of particle.

Question 52

define element

Answer 52

a pure substance which cannot be further broken down by ordinary chemical means.

Question 53

define isotope.

Answer 53

atoms of the same elements which differ in the number of neutrons.

Question 54

define mass number

Answer 54

corresponds to the total number of particles present in the nucleus of a single atom.

Question 55

define radioisotope

Answer 55

a radioactive isotope.

Question 56

define isotopic abundance.

Answer 56

the relative amount in which each isotope is present in an element.

Question 57

define valence number.

Answer 57

identifies the number of electrons which the atom must gain or lose in order to have its outer energy level filled.

Question 58

define average atomic mass.

Answer 58

a number which represents the average weighted mass of all the isotopes of that element.

Question 59

define screening electrons.

Answer 59

the electrons found in the inner orbits between the nucleus and the valence electrons.

Question 60

what are the 6 steps of the scientific method?

Answer 60

1. Identify the problem. 2. Propose a solution to the problem. 3. Test the proposed solution through experimentation. 4. Gather data using the senses. 5. Analyse the data using the brain. 6. Formulate conclusions.

Question 61

what is the mass of proton, electron and neutron particles?

Answer 61

proton: 1u electron: 1/1837u neutron: 1u

Question 62

name 3 general properties of metals.

Answer 62

-metals are generally lustrous (shiny) -metals are very good conductors of both heat and electricity -metals are both ductile and malleable.

Question 63

name 3 general properties of non-metals.

Answer 63

-nonmetals are normally dull in appearance -nonmetals are poor conductors of heat and electricity -nonmetals do not bend they are considered to be brittle

Question 64

what is the law of periodicity?

Answer 64

when elements are arranged in order of increasing atomic number, there is a periodic repetition of elements with similar properties.

Question 65

explain an ionic bond.

Answer 65

forms when electrons are completely transferred from one atom to another.

Question 66

explain a covalent bond.

Answer 66

forms when electrons are shared between atoms.

Question 67

what are the two main purposes of the IUPAC nomenclature system?

Answer 67

1. To provide a nomenclature that would be recognized internationally so that chemists around the world could effectively communicate with one another. 2. To provide a systematic approach to naming chemicals so that new compounds could easily be named according to existing nomenclature.