CHEM Flashcards
What is the atomic number of Carbon?
6
True or False: The Periodic Table is organized by increasing atomic mass.
False
Fill in the blank: The element with the symbol ‘Na’ is called ______.
Sodium
Which group of the Periodic Table contains the noble gases?
Group 18
What is the chemical symbol for Gold?
Au
True or False: All elements in the same group have similar chemical properties.
True
What does the term ‘period’ refer to in the Periodic Table?
A horizontal row of elements.
What is the most abundant element in the universe?
Hydrogen
Which element has the highest atomic number currently known?
Oganesson (Og)
Fill in the blank: The elements in Group 1 are known as ______ metals.
Alkali
What is the main characteristic of transition metals?
They can form variable oxidation states.
Which element is represented by the symbol ‘Fe’?
Iron
What is the periodic law?
The properties of elements are periodic functions of their atomic numbers.
Which two elements are liquid at room temperature?
Mercury and Bromine
True or False: Helium is a reactive gas.
False
What is the difference between an element and a compound?
An element is a pure substance made of one type of atom; a compound is made of two or more different types of atoms chemically bonded.
What is the main characteristic of metalloids?
They have properties of both metals and nonmetals.
Which group contains the alkali earth metals?
Group 2
What is the chemical symbol for Silver?
Ag
Fill in the blank: The first element in the Periodic Table is ______.
Hydrogen
How many periods are there in the modern Periodic Table?
7
What type of bond is formed between two nonmetals?
Covalent bond
True or False: Nonmetals are good conductors of electricity.
False
Which element is a gas at room temperature and has the atomic number 7?
Nitrogen
What is the primary use of the element Silicon?
Semiconductors in electronics.
Which element is represented by the symbol ‘K’?
Potassium
Fill in the blank: The most reactive group of nonmetals is the ______.
Halogens
What is ionisation energy?
The energy required to remove an electron from an atom or ion in its gaseous state.
True or False: Ionisation energy increases across a period in the periodic table.
True
What trend in ionisation energy is observed down a group in the periodic table?
Ionisation energy decreases.
Which element has the highest ionisation energy in the periodic table?
Helium
Fill in the blank: The first ionisation energy is the energy required to remove the _____ electron from a neutral atom.
first
What is the general trend of ionisation energy as atomic number increases within a group?
It generally decreases.
Multiple Choice: Which of the following elements has the lowest first ionisation energy? A) Lithium B) Barium C) Neon D) Fluorine
B) Barium
What is the second ionisation energy?
The energy required to remove a second electron from a singly charged ion.
True or False: Ionisation energy is always a positive value.
True
Which factors influence ionisation energy?
Nuclear charge, electron shielding, and atomic radius.
Fill in the blank: Ionisation energy is typically measured in _____ per mole.
kilojoules
What is meant by ‘successive ionisation energies’?
The energies required to remove each electron in turn from an atom or ion.
Multiple Choice: Which of the following elements would you expect to have a higher ionisation energy? A) Sodium B) Chlorine
B) Chlorine
What happens to the ionisation energy of an atom as it becomes positively charged?
The ionisation energy increases.
True or False: The first ionisation energy is typically lower than the second ionisation energy.
True
What is the relationship between ionisation energy and the reactivity of metals?
Lower ionisation energy typically indicates higher reactivity.
Fill in the blank: The trend of ionisation energy can be explained by _____ theory.
atomic structure
Multiple Choice: Which of the following has the highest second ionisation energy? A) Magnesium B) Sodium C) Potassium D) Calcium
A) Magnesium
What is the significance of a large jump in successive ionisation energies?
It indicates a change in the electron shell or a more stable electron configuration.
True or False: Noble gases have high ionisation energies.
True
What is the effect of electron shielding on ionisation energy?
Electron shielding reduces the effective nuclear charge felt by outer electrons, lowering ionisation energy.
What does a high ionisation energy imply about an element’s ability to lose electrons?
It implies that the element has a low tendency to lose electrons.
Fill in the blank: The ionisation energy of an element can be affected by its _____ state.
oxidation
Multiple Choice: Which group of elements generally has low ionisation energies? A) Alkali metals B) Noble gases C) Halogens D) Transition metals
A) Alkali metals
What is the unit of measurement for ionisation energy?
Kilojoules per mole (kJ/mol).
